{"id":4482,"date":"2022-03-13T16:49:28","date_gmt":"2022-03-13T11:19:28","guid":{"rendered":"https:\/\/devinfinitylearn.in\/surge\/chemical-equilibrium-questions-for-cbse-class-11th\/"},"modified":"2022-03-13T16:49:28","modified_gmt":"2022-03-13T11:19:28","slug":"chemical-equilibrium-questions-for-cbse-class-11th","status":"publish","type":"post","link":"https:\/\/devinfinitylearn.in\/surge\/chemistry\/chemistry-questions\/chemical-equilibrium\/","title":{"rendered":"Chemical Equilibrium Questions for CBSE Class 11th"},"content":{"rendered":"

Which one of the following statements is incorrect about chemical equilibrium?<\/a><\/p>\n

For the reversible reaction, A \u21cc \u2009 2 B , K c = 10 . At certain instant, [A] = 2M and [B] = 200M. Then the correct statement is<\/a><\/p>\n

The vapour pressure of a liquid in a closed container depends on : (1) temperature of liquid (2) quantity of liquid (3) surface area of the liquid<\/a><\/p>\n

Correct statement among the following is<\/a><\/p>\n

In the decomposition of PCl 5 , the degree of decomposition of PCl 5 is 0.5. If initially 2 moles of PCl 5 is taken in a 2 litre vessel, the value of K p at an equilibrium pressure of 2 atm is<\/a><\/p>\n

A 10 litre container at 400K contains CO 2 g at 0.1 atm and an excess solid metal oxide, MO. The volume of the container is now decreased by moving the movable piston fitted to the container. Maximum volume of the container when the pressure of CO 2 attains its maximum value will be MCO 3 ( s ) \u21cc MO ( s ) + CO 2 ( g ) ; ( K p = 0.8 atm)<\/a><\/p>\n

At 500 K, equilibrium constant, K c , for the following reaction is 5. 1 2 H 2 g + 1 2 I 2 g \u21cc HI g What would be the equilibrium constant K c for the reaction? 2 HI g \u21cc H 2 g + I 2 g<\/a><\/p>\n

Predict which of the following reaction will have appreciable concentration of reactants and products?<\/a><\/p>\n

Which of the following is the example of a reversible reaction?<\/a><\/p>\n

In the reaction, C ( s ) + CO 2 ( g ) \u21cc 2 CO ( g ) , when pressure is increased, the reaction goes in the<\/a><\/p>\n

K a 1 , K a 2 and K a 3 are the respective ionisation constants for the following reactions. H 2 S \u21cc H + + HS – HS – \u21cc H + + S 2 – H 2 S \u21cc 2 H + + S 2 – The correct relationship between K a 1 , K a 2 , K a 3 is<\/a><\/p>\n

The value of K c for the reaction 2 A \u21cc B + C is 2 \u00d7 10 – 3 . At a given time, the composition of the mixture is A = B = C = 3 \u00d7 10 – 4 M . Identify correct statement about the equllibrium system.<\/a><\/p>\n

Attainmenet of “equilibrium state” with the help of “constancy in intensity of colour” is noticed in the case of following reaction occuring in a closed vessel<\/a><\/p>\n

Which of the following is an irreversible reaction.<\/a><\/p>\n

The reaction is reversible if it is carried out<\/a><\/p>\n

When H 2 and I 2 are mixed and equilibrium is attained, then<\/a><\/p>\n

Regarding a catalyst some statements are given below. Correct statement among the following is<\/a><\/p>\n

When the rate of formation of reactants is equal to the rate of formation of products, this is known as,<\/a><\/p>\n

The following are some statements about equilibrium constant. (A) Equilibrium constant is influenced by temperature change (B) Value of equilibrium constant gives an idea about the extent of completion of reaction (C) Equilibrium constant is influenced by volume and pressure changes The correct combination is.<\/a><\/p>\n

At a given temperature, for a reversible reaction, if the concentration of reactants is doubled then the equilibrium constant will<\/a><\/p>\n

1) 2) 3) 4) From the above data, the most stable oxide is<\/a><\/p>\n

The reaction is carried out in a litre flask. If the same reaction is carried out in a 2 litre flask at the same temperature, the equilibrium constant will be<\/a><\/p>\n

K C for is 'K', then for , it is<\/a><\/p>\n

The equilibrium constants for the following reactions are K 1 and K 2 respectively, equilibrium constant for the following reaction will be<\/a><\/p>\n

The reaction which goes farthest to completion is<\/a><\/p>\n

The equilibrium constant, K p for the gaseous reaction A \u21cc 2B is related to degree of dissociation ( \u03b1 ) of A and total pressure P as<\/a><\/p>\n

For this reaction the value of K p K c will be<\/a><\/p>\n

With increase in temperature generally the value of the equilibrium constant of endothermic reversible reaction<\/a><\/p>\n

A gas bulb is filled with NO 2 gas and immersed in an ice bath at 0 0 C which becomes colourless after sometime. This colourless gas will be<\/a><\/p>\n

If pressure is increased on the equilibrium, ice \u21cc water<\/a><\/p>\n

A liquid is in equilibrium with its vapour at its boiling point.The molecules in the two phases have equal<\/a><\/p>\n

For the gaseous reaction as per Lechatelier’s principle which of the following changes favour forward reaction yielding more sulphur trioxide ? A) Adding more oxygen B) Removing sulphur trioxide C) Applying high pressure D) presence of catalyst<\/a><\/p>\n

At 298K, the equilibrium constant for a reaction is 100. If the initial concentration of each species is 1M, the equilibrium concentration of D in molL – 1 is<\/a><\/p>\n

The equilibrium constant for the given reaction is 100. What is the equilibrium constant for the reaction given : at same temperature is<\/a><\/p>\n

4g H 2 and 127g I 2 are mixed & heated in 10 lit closed vessel until equilibrium is reached. If the equilibrium concentration of HI is 0.05 M, total number of moles present at equilbrium is<\/a><\/p>\n

At a given temperature, K c is 4 for the reaction . Initially 0.6 moles each of H 2 and CO 2 are taken in 1lit flask. The equilibrium concentration of H 2 O (g) is<\/a><\/p>\n

A mixture of 2 moles of N 2 and 8 moles of H 2 are heated in a 2 lit vessel, till equilibrium is established. At equilibrium, 0.4 moles of N 2 was present. The equilibrium concentration of H 2 will be<\/a><\/p>\n

At constant temperature 80% AB dissociates into A 2 and B 2 , then the equillibrium constant for is<\/a><\/p>\n

For the gaseous reaction, A + B \u21cc C + D , the initial concentration of \u2018A\u2019 and \u2018B\u2019 are equal. The equilibrium concentration of \u2018C\u2019 is half the initial concentration of \u2018A\u2019. The equilibrium constant for the reaction is<\/a><\/p>\n

1.0 mole of ethyl alcohol and 1.0 mole of acetic acid are mixed. At equilibrium, 0.666 mole of ester is formed. The value of equilibrium constant is<\/a><\/p>\n

9.2g of N 2 O 4(g) is taken in 1lit vessel and heated. At equilibrium, 50% is dissociated. Equilibrium constant in (mol\/lit) for the reaction N 2 O 4(g) \u21cc 2NO 2(g) is<\/a><\/p>\n

For , , K f and K b respectively are 0.25 and 5000 at 400K. Now, K c for same process at 500K may be<\/a><\/p>\n

\u2018x\u2019 moles of N 2 O 4 is taken at P 1 atm in a closed vessel & heated. When 75% of N 2 O 4 dissociated at equilibrium, total pressure at equilibrium was found to be P 2 atm. The relation between P 1 and P 2 is<\/a><\/p>\n

For , continuous removal of NH 3 maintains the following condition<\/a><\/p>\n

A vessel contains N 2 O 4 & NO 2 in 2:3 molar ratio at 10 atm under equilibrium. Now, K P for is<\/a><\/p>\n

20 gm of CaCO 3 is allowed to dissociate in a 5.6 litre container at 819 0 C. If 50% of CaCO 3 is dissocitated at equilibrium, the 'K p ' value is<\/a><\/p>\n

When the molar concentrations of SO 2 , O 2 and SO 3 at equilbrium at certain temperature are 0.5, 0.25 & 0.25M respectively, K C for is<\/a><\/p>\n

N 2 O 4 at an initial pressure of 2atm. and 300k dissociates to an extent of 20% at the same temperature by the time equilibrium is established. K p for the reaction 2NO 2 \u21cc N 2 O 4 is<\/a><\/p>\n

Some amount of solid NH 4 HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. Ammonium hydrogen sulphide decomposes to yield NH 3 and H 2 S gases in the flask. When the decomposition reaction reaches equilibrium the total pressure in the flask rises to 0.84 atm. The equilibrium constant for NH 4 HS decomposition at this temperature is<\/a><\/p>\n

For the gaseous phase reaction , initially there are 2 mole each of A&B. If 0.4 mol of D is present at equilibrium at a given T & P, incorrect relationship is<\/a><\/p>\n

For at equilibrium, , where P is equilibrum pressure. Then degree of dissociation of PCl 5 at that temperature is<\/a><\/p>\n

If the percentage dissociation of N 2 O 4 is 50, the ratio of Kp and P eq for N 2 O 4 \u21cc 2 NO 2 becomes equal to<\/a><\/p>\n

For the reaction at 900K, the equilibrium steam-hydrogen mixture was found to be 40% H 2 by volume. The K P is<\/a><\/p>\n

The vapour density of N 2 O 4 at certain temperature is 30. What is the percentage dissociation of N 2 O 4 at that temperature?<\/a><\/p>\n

140 mm pressure is developed at equilibrium when PCl 5 at 100mm is subjected to dissociation. Then K P for PCl 3 +Cl 2 \u21cc PCl 5 is (in atm -1 ) nearly<\/a><\/p>\n

20% of N 2 O 4 molecules are dissociated in a sample of gas at 27ºC and 760 torr. Mixture has the density at equilibrium equal to<\/a><\/p>\n

Equilibrium constant depends on<\/a><\/p>\n

Consider the following statements. I. In general, the temperature dependence of the equilibrium constant depends on the sign of \u2206 H for the reaction. II. The equilibrium constant for an exothermic reaction (negative, \u2206 H )decreases as the temperature increases. III. The equilibrium constant for an endothermic reaction (positive, \u2206 H )increases as the temperature increases. IV. Temperature changes affect the equilibrium constant and rates of reactions. Choose the correct statements.<\/a><\/p>\n

Match the Column I with Column II and choose the correct option from the codes given below. Column I (Process) Column II (Conclusion) A. Liquid \u21cc vapour 1. Concentration of solute in solution is constant at a given temperature. B. Solid \u21cc liquild 2. [ Gas ( aq ) ] [ Gas ( s ) ] is – constant at a given temperature. C. Solute ( S ) \u21cc solute ( solution ) 3. P H 2 O constant at given temperature D. Gas ( g ) \u21cc Gas ( aq ) 4. Melting point is fixed at constant pressure. Codes<\/a><\/p>\n

A 10 litre closed vessel contains 5 moles of nitrogen, 10 moles of hydrogen and 10 moles of ammonia at equilibrium. Equilibrium constant for the reaction N 2 + 3 H 2 \u21cc 2 NH 3 is<\/a><\/p>\n

The equilibrium constant for a reaction is K, and the reaction quotient is Q. For a particular reaction mixture, the ratio K Q is 0.33 This means that<\/a><\/p>\n

The equilibrium constant Kc for the following reaction at 842 o C is 7.90 x 10 -3 .What is K p at same temperature? 1 2 F 2 ( g ) \u21cc F ( g )<\/a><\/p>\n

A catalyst is a substance which :<\/a><\/p>\n

What will be the effect on the equilibrium constant on increasing temperature , if the reaction neither absorbs heat nor releases heat?<\/a><\/p>\n

An equilibrium mixture of the reaction 2 H 2 S ( g ) \u21cc 2 H 2 ( g ) + S 2 ( g ) had 0.5 mole H 2 S, 0.10 mole H 2 and 0.4 mole S 2 in one liter vessel. The value of equilibrium constant (K) in mol litre -1 is<\/a><\/p>\n

The equilibrium constant for the following reaction is 10.5 at 500 K. A system at equilibrium has [ CO ] = 0 . 250 M and H 2 = 0 . 120 M what is the CH 3 OH ? CO ( g ) + 2 H 2 ( g ) \u21cc CH 3 OH ( g )<\/a><\/p>\n

One mole of pure ethyl alcohol was treated with one mole of pure acetic acid at 25 o C. One-third of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be :<\/a><\/p>\n

when heated, ammonium carbamate decomposes as follows NH 4 COONH 2 ( s ) \u21cc 2 NH 3 ( g ) + CO 2 ( g ) At a certain temperature, the equilibrium pressure of the system is 0.318 arm. K p for the reaction is :<\/a><\/p>\n

5 Moles of SO 2 and 5 moles of O 2 are allowed to react. At equilibrium, it was found that 60% of SO 2 is used up. If the pressure of the equilibrium mixture is one atmosphere, the partial pressure of O 2 is<\/a><\/p>\n

Pure PCl 5 is introduced into an evacuated chamber and comes to equilibrium at 247 o C and 2.0 atm. The equilibrium gaseous mixture contains 40% chlorine by volume. Calculate K p at 247 \u2218 C for the reaction PCl 5 ( g ) \u21cc PCl 3 ( g ) + Cl 2 ( g )<\/a><\/p>\n

For the reaction XCO 3 ( s ) \u21cc XO ( s ) + CO 2 ( g ) , K p = 1 .642 atm at 727 \u2218 C . If 4 Mole of XCO 3 ( s ) was put into a 50 liter container and heated to 727 O C What mole percent of the XCO 3 , remains unreacted at equilibrium?<\/a><\/p>\n

Bond dissociation energies of following reactios is given below A – B A \u2219 + B \u2219 ; \u2206 H 1 A – B A \u2295 + B \u229d ; \u2206 H 2 Identify correct relation(magnitude only)<\/a><\/p>\n

The volume of the reaction vessel containing an equilibrium mixture is increased in the following reaction SO 2 Cl 2 ( g ) \u21cc SO 2 ( g ) + Cl 2 ( g ) When equilibrium is re-established :<\/a><\/p>\n

The graph which represents all the equilibrium concentrations for the reaction N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) Then the select the correct graph for concentrations of NO 2 against concentrations of N 2 O 4<\/a><\/p>\n

The vapour pressure of mercury is 0.002 mm Hg at 27 \u2218 C . K c for the process Hg ( l ) \u21cc Hg ( g ) is<\/a><\/p>\n

For which of the following equilibria is K c = K p<\/a><\/p>\n

Le-Chatelier principle is not applicable to :<\/a><\/p>\n

Consider the following reaction and determine which of the conditions will shift the equilibrium position to the right? 4 NH 3 ( g ) + 5 O 2 ( g ) \u21cc 4 NO ( g ) + 6 H 2 O ( g ) + Heat<\/a><\/p>\n

For the equilibrium reaction NH 4 HS (s) \u21cc NH 3(g) +H 2 S (g) K p at a given temperature is 25 atm 2 . Total pressure at equilibrium is<\/a><\/p>\n

For which one of the following reaction at equilibrium constant value increases with decrease in temperature.<\/a><\/p>\n

The value of \u2206 G \u00b0 for a reaction in aqueous phase having K c = 1, would be:<\/a><\/p>\n

For a given exothermic reaction K p and K p ‘ are the equilibrium constants at temperatures T 1 a n d T 2 , respectively. Assuming that heat of reaction is constant in temperature range between T 1 a n d T 2 , it is readily observed that<\/a><\/p>\n

If the value of equilibrium constant for a particular reaction is 1 . 6 \u00d7 10 12 , then at equilibrium the system will contain<\/a><\/p>\n

A ) \u2009\u2009 2 KMnO 4 \u2009\u2009 \u2009\u2009 K 2 MnO 4 + MnO 2 + O 2 B ) \u2009\u2009 2 NaNO 3 \u2009 2 NaNO 2 + O 2 Correct statement regarding the above reactions is<\/a><\/p>\n

A 10 litre closed vessel contains 2 moles of nitrogen, 5 moles of hydrogen and 10 moles of ammonia at equilibrium. Equilibrium constant for the reaction N 2 + 3 H 2 \u21cc 2 NH 3 is<\/a><\/p>\n

A 2 g \u2009\u2009 + \u2009 B 2 g \u2009 \u21cc \u2009\u2009 3 X 2 g , \u2009\u2009\u2009 \u0394H = + XkJ \u2009\u2009 According to Lechatelier’s principle, favourable conditions for the decomposition of X 2 are<\/a><\/p>\n

is an example of …<\/a><\/p>\n

Change in volume of the system does not alter the number of moles in which of the following equilibrium ?<\/a><\/p>\n

The following are some statements about equilibrium state A) The rate of forward reaction is equal to the rate of backward reation. B) The chemical equilibrium can be established from reactant side only C) The concentration of the reactants and products remain constant with time. The correct statements are<\/a><\/p>\n

A vessel (A) contains 1 mole each of N 2 and O 2 and another vessel (B) contains 2 mole each of N 2 & O 2 . Both vessels are heated to same temperature till equilibrium is established in both cases. Then, correct statement is<\/a><\/p>\n

Law of mass action is applicable to a) Chemical reactions [Reversible] b) Chemical reactions [Irreversible] c) Homogeneous equilibria and heterogeneous equilibria d) Physical equilibria<\/a><\/p>\n

The following are some statements about active masses. A) Active mass of pure liquids and solids are taken as unity. B) Active mass of electrolytes is taken as molality. C) For dilute solutions of non-electrolytes, the active mass can be taken as molarity. The correct combination is.<\/a><\/p>\n

Which one of the following has greater active mass?<\/a><\/p>\n

For the chemical reaction the amount of AB at equilibrium is affected by<\/a><\/p>\n

Starting from 'a' moles of H 2 and 'b' moles of I 2 an equilibrium is established with 2x moles of HI. The equilibrium constant K C is<\/a><\/p>\n

The following equilibria are given The equilibrium constant of the reaction, in terms of K 1 , K 2 and K 3 will be<\/a><\/p>\n

The equilibrium constant for the reaction , CaSO 4 . 5 H 2 O s \u21cc CaSO 4 . 3 H 2 O s + 2 H 2 O g , is equal to<\/a><\/p>\n

Which of the following expression is true for the system ?<\/a><\/p>\n

For which of the following reactions, the degree of dissociation ( \u03b1 ) and equilibrium constant (K p ) are related as k p = 4 \u03b1 2 p 1 – \u03b1 2 ?<\/a><\/p>\n

Correct relation between K p and K c for this reaction is<\/a><\/p>\n

A reversible chemical reaction having two reactants in equilibrium. If the concentration of the reactants are doubled, then the equilibrium constant will<\/a><\/p>\n

For the physical equilibrium, ice \u21cc water , the forward reaction is not favoured by<\/a><\/p>\n

A reaction is at equilibrium. If the concentration of N 2 is increased the temperature of the system<\/a><\/p>\n

At equilibrium the concentration of ‘B’ is doubled. By what factor the concentration of ‘D’ should increase to retain the equilibrium<\/a><\/p>\n

In the reaction ; . On increasing the temperature the production of NO<\/a><\/p>\n

Exothermic formation represented by equation kJ. Which of the following will increase the quantity of ClF 3 in equilibrium mixture ?<\/a><\/p>\n

Of the following, which change will shift the reaction towards the product I 2 ( g ) \u21cc 2 I ( g ) , \u0394H 0 f ( 298 K ) = + 150 kJ<\/a><\/p>\n

Which one of the following statements about physical equilibrium is incorrect ?<\/a><\/p>\n

Wrong statement about equilibrium state is<\/a><\/p>\n

In which of the following reactions, the equilibrium remains unaffected on addition of small amount of argon at constant volume?<\/a><\/p>\n

Solubility of gases in liquids is maximum at<\/a><\/p>\n

Active mass of 0.64 g SO 2 in 10 lit vessel is<\/a><\/p>\n

The equilibrium constant for the reaction is 2 at a certain temp. The equilibrium concentrations of both H 2 and HI are 2 mol.lit -1 . What is the equilibrium concentra-tion (in mole.lit 1 ) of I 2 ?<\/a><\/p>\n

If equilbrium concentration of each component is 0.2M, correct order of K c of:<\/a><\/p>\n

Active mass of 5.6 lit nitrogen at STP<\/a><\/p>\n

Initially 0.8 mole of PCl 5 and 0.2 mole of PCl 3 are mixed in one litre vessel. At equilibrium 0.4 mole of PCl 3 is present. The value of K C for the reaction<\/a><\/p>\n

A mixture of 0.3 mole of H 2 and 0.3 mole of I 2 is allowed to react in a 10 lit vessel at 500 0 C. If K C of is 64, the amount of unreacted I 2 at equilibrium is<\/a><\/p>\n

. This reaction is performed in a 1 lit vessel. Equilibrium is established when 0.5 mole of benzene is present at certain temperature. If equilibrium constant is 4 lit 2 mole -2 . The total number of moles of the substances present at equilibrium.<\/a><\/p>\n

HI was heated in a sealed tube at 440 0 C till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for the dissociation of HI is<\/a><\/p>\n

A (g) + 3B (g) \u21cc 4C (g) . Initial concentration of A is equal to that of B. The equilibrium concentration of A and C are equal. K C is equal to<\/a><\/p>\n

1.2 moles of SO 3 are allowed to dissociate in a 2 litre vessel the reaction is and the concentration of oxygen at equilibrium is 0.1 mole per litre. The total number of moles at equilibrium will be<\/a><\/p>\n

For A + B \u21cc C , the equilibrium concentrations of A and B at a temperature are 15 mole\/lit. When volume is doubled the reaction has equilibrium concentration of A as 10 mol\/lit. The concentration of C in original equilibrium is<\/a><\/p>\n

One mole of a compound AB reacts with one mole of a compound CD according to the equation . When equilibrium had been established it was found that 3 4 mole of reactants AB and CD had been converted to AD and CB. There is no change in volume. The equilibrium constant for the reaction is<\/a><\/p>\n

An equilibrium mixture for the reaction has one mole of hydrogen sulphide, 0.2 mole of H 2 and 0.8 mole of S 2 in a 2 litre vessel. The value of K C in mole litre -1 is<\/a><\/p>\n

1 mole A (g) is heated in 1lit closed vessel and equilibrium is reached at 300 0 C in A (g) \u21cc B (g) . If K C = 4, concentration of B (g) at equilibrium is (in mole\/lit)<\/a><\/p>\n

For the reaction , the concentrations of A and B are equal. The equilibrium concentration of C is twice that of A. K C of the reaction is<\/a><\/p>\n

For the gaseous reaction , the equilibrium pressures of H 2 and N 2 are 0.4 atm and 0.8 atm respectively. The total pressure of the equilibrium system is 2.8 atm. The value of K p is<\/a><\/p>\n

A vessel at 1000 K contains CO 2 with a pressure of 0.5 atm. Some of CO 2 is converted into CO on addtion of graphite. The value of ‘K’ at equilibrium for the reaction, CO 2 g + C s \u21cc 2 CO g , when total pressure is 0.8 atm will be<\/a><\/p>\n

Kp value for is 5.0 atm -1 . What is the equilibrium partial pressure of O 2 if the equilibrium pressures of SO 2 and SO 3 are equal ?<\/a><\/p>\n

In a closed container and at constant temperature 0.3 mole of SO 2 and 0.2 mole of O 2 gas at 750 torr are kept with a catalyst. If at equilibrium 0.2 mole of SO 3 is formed the partial pressure of SO 2 is …….. torr<\/a><\/p>\n

A mixture of Nitrogen and Hydrogen is at an initial pressure of 200atm. If 20% of the mixture reacts by the time equilibrium is reached, the equilibrium pressure of the mixture is<\/a><\/p>\n

A vessel contains 1 mole PCl 5 (g) at 4 atm and 0.5 mole PCl 3 formed at equilibrium. Now, equilibrium pressure of mixture is (assume ideal behavior)<\/a><\/p>\n

P eq for at certain temperature is 0.9 atm. Then, partial pressure of ammonia at equilibrium (in atm)<\/a><\/p>\n

For the following reaction , the total pressure at equilibrium is 30 atm. The value of Kp is<\/a><\/p>\n

K C for in a 10 lit flask at certain T is 100 lit-mol -1 . Now, if equilibrium pressures of SO 2 and SO 3 are equal, then mass of O 2 present at equilibrium is<\/a><\/p>\n

At a certain temperature and a total pressure of 10 5 Pa, iodine vapours contain 40% by volume of iodine atoms at equilibrium I 2 ( g ) \u21cc 2 I ( g ) K P for the equilibrium will be<\/a><\/p>\n

Ammonium carbamate when heated to 200ºC gives a mixture of NH 3 and CO 2 vapour with a density of 13. What is the degree of dissociation of ammonium carbamate?<\/a><\/p>\n

Dissociation constant of water at 25 0 C is<\/a><\/p>\n

Statement I : If Q c (Reaction quotient) < K C (equilibrium constant) reaction moves in direction of reactants. Statement II : Equilibrium constant is defined in the same way as reaction quotient at end stage of the reaction.<\/a><\/p>\n

Statement I : Introduction of catalyst does not affect position of equlibrium Statement II : For a reversible reaction, presence of a catalyst influences both forward & backward reaction to the same extent<\/a><\/p>\n

For the equilibrium reaction PCl 5(g) \u21cc PCl 3(g) + Cl 2(g) ; K c at 360 K is 0.01 mole\/lit. K p for the same reaction at same temperature is<\/a><\/p>\n

The expression for the equilibrium constant for gaseous reaction is K c = NH 3 4 O 2 5 NO 4 H 2 O 6 . Identify the correct balanced chemical equation corresponding to this expression<\/a><\/p>\n

When no more of solute can be dissolved in a solution at a given temperature, the solution is called<\/a><\/p>\n

A mixture of reactants and products in the state of equilibrium is called<\/a><\/p>\n

I H 2 g + I 2 g \u21cc 2 HI g ; K C is eqm . constt . ( II ) 2 HI ( g ) \u21cc H 2 ( g ) + I 2 ( g ) ; K C ‘ is eqm . constt . How are K C and K C ‘ related to each other ?<\/a><\/p>\n

Which of the following condition will favour the formation of NH 3 by Haber process? N 2 g + 3 H 2 g \u21cc 2 NH 3 g ; – 92 . 38 kJ mol – 1<\/a><\/p>\n

For a hypothetical reaction, 2 A g \u21cc B g , at 300 K , the correct relation is<\/a><\/p>\n

According to Lechatlier principle, decomposition of PCl 5 (g) is favoured at<\/a><\/p>\n

Which of the following will not change the concentration of ammonia in the equilibrium? 4 NH 3 ( g ) + 5 O 2 ( g ) \u21cc 4 NO ( g ) + 6 H 2 O ( l ) , \u0394H = + ve<\/a><\/p>\n

Hydrolysis of sucrose gives, Sucrose + H 2 O \u21cc Glucose + Fructose Equilibrium constant K C for the reaction is 2 \u00d7 10 13 at 300 K . Calculate \u0394G \u00b0 at 300 K .<\/a><\/p>\n

Based on the extent to which the reactions proceed to reach the state of chemical equilibrium, the reactions may be classified I. The reactions that proceed nearly to completion and only negligible concentrations of the reactants are left. II. The reactions in which only small amounts of products are formed and most of the reactants remain unchanged at equilibrium stage. III. The reactions in which the concentrations of the reactants and products are comparable, when the system is in equilibrium Which of the following is correct option?<\/a><\/p>\n

Statement I: When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium mixture changes, so as to minimize the effect of concentration changes. Statement II: It illustrates Le-chatelier’s principle on the effect of concentration change.<\/a><\/p>\n

Calculate the partial pressure of carbon monoxide from the following data CaCO 3 ( s ) \u21cc \u0394 CaO ( s ) + CO 2 ( g ) ; K p = 8 \u00d7 10 – 2 CO 2 ( g ) + C ( s ) \u21cc 2 CO ( g ) ; K p = 2<\/a><\/p>\n

Identify correct statements among the following A) A catalyst cannot influence equilibrium state B) At equilibrium, \u2206 G is always zero C) Law of mass action is applicable to chemical process only D) When Q c < K c , backward reaction is favoured<\/a><\/p>\n

Consider the reaction 2 SO 2 ( g ) + O 2 ( g ) \u21cc 2 SO 3 ( g ) for which K c = 278 M – 1 \u00b7 0 . 001 Mole of each of the reagents SO 2 ( g ) , O 2 ( g ) and SO 3 ( g ) are mixed in a 1.0 L flask. Determine the reaction quotient of the system and the spontaneous direction of the system :<\/a><\/p>\n

The figure shows the change in concentration of species A and B as a function of time The equilibrium constant K c for the reaction A ( g ) \u21cc 2 B ( g ) is<\/a><\/p>\n

Using molar concentrations, what is the unit of K c . for the reaction? CH 3 OH ( g ) \u21cc CO ( g ) + 2 H 2 ( g )<\/a><\/p>\n

For the reaction CO ( g ) + Cl 2 ( g ) \u21cc COCl 2 ( g ) the value of K c K p is equal to<\/a><\/p>\n

The concentration of a pure solid or liquid phase is not included in the expression of equilibrium constant because :<\/a><\/p>\n

For the reaction 2 NO 2 ( g ) + 1 2 O 2 ( g ) \u21cc N 2 O 5 ( g ) if the equilibrium constant is K p , then the equilibrium constant for the reaction 2 N 2 O 5 ( g ) \u21cc 4 NO 2 ( g ) + O 2 ( g ) would be:<\/a><\/p>\n

At a certain temperature, the following reactions have the equilibrium constants as shown below: S ( s ) + O 2 ( g ) \u21cc SO 2 ( g ) ; K c = 5 \u00d7 10 52 2 S ( s ) + 3 O 2 ( g ) \u21cc 2 SO 3 ( g ) ; K c = 10 29 What is the equilibrium constant Kc for the reaction at the same temperature ? 2SO 2 ( g ) + O 2 ( g ) \u21cc 2 SO 3 ( g )<\/a><\/p>\n

Consider the following gaseous equilibria given below: (I) N 2 + 3 H 2 \u21cc 2 NH 3 ; Eqm. Constant = K 1 (II) N 2 + O 2 \u21cc 2 NO ; Eqm. Constant = K 2 (III) H 2 + 1 2 O 2 \u21cc H 2 O ; Eqm. Constant = K 3 The equilibrium constant for the reaction, 2 NH 3 + 5 2 O 2 \u21cc 2 NO + 3 H 2 O in terms of K 1 , K 2 and K 3 will be<\/a><\/p>\n

Given CS 2 = 0 . 120 M , H 2 = 0 . 10 M , H 2 S = 0 . 20 M and CH 4 = 8 . 40 \u00d7 10 – 5 M for the following reaction at 900 o C, at eq. Calculate the equilibrium constant K c CS 2 ( g ) + 4 H 2 ( g ) \u21cc CH 4 ( g ) + 2 H 2 S ( g )<\/a><\/p>\n

When sulphur (in the form of S 8 ) is heated at temperature T at equilibrium, the pressure of S 8 falls by 30% from 1.0atm, because S 8 (g) is partially converted into S 2 (g). Find the value of K p for this reaction.<\/a><\/p>\n

For the reaction 2A (g) \u21cc B ( g ) + 3 C ( g ) at a given temperature, K c = 16 What must be the volume of the flask, if a mixture of 2 mole each of A, B and C exist in equilibrium?<\/a><\/p>\n

I 2 ( aq ) + I – ( aq ) \u21cc I 3 – ( aq ) We started with 1 mole of l 2 and 0.5 mole of I – in one liter flask. After equilibrium is reached, excess of Ag NO 3 gave 0.25 mole of yellow precipitate. Equilibrium constant is :<\/a><\/p>\n

In the equilibrium SO 2 ( g ) + O 2 ( g ) \u21cc 2 SO 3 ( g ) the partial pressure of SO 2 , O 2 and SO 3 are 0.662,0.10 and 0.331atm respectively What should be the partial pressure of oxygen so that the equilibrium concentrations of SO 2 and SO 3 are equal?<\/a><\/p>\n

In a system A ( s ) \u21cc 2 B ( g ) + 3 C ( g ) if the concentration of C at equilibrium is increased by a factor of 2, it will cause the equilibrium concentration of B to change to :<\/a><\/p>\n

At a certain temperature, only 50% HI is dissociated at equilibrium in the following reaction : 2 HI ( g ) \u21cc H 2 ( g ) + I 2 ( g ) The equilibrium constant for this reaction is :<\/a><\/p>\n

0.1 Mole of N 2 O 4 ( g ) was sealed in a tube under one atmospheric conditions at 25 o C. Calculate the number of moles of NO 2 ( g ) present, if the equilibrium N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) K p = 0 .14 is reached after some time :<\/a><\/p>\n

At a certain temperature the equilibrium constant K c is 0.25 for the reaction A 2 ( g ) + B 2 ( g ) \u21cc C 2 ( g ) + D 2 ( g ) If we take 1 mole of each of the four gases in a 10 litre container, what would be equilibrium concentration of A 2 ( g ) ?<\/a><\/p>\n

At 200 O C PCl 5 . dissociates as follows : PCl 5 ( g ) \u21cc PCl 3 ( g ) + Cl 2 ( g ) It was found that the equilibrium vapors are 62 times as heavy as hydrogen. The % degree of dissociation of PCl 5 at 200 o C is nearly :<\/a><\/p>\n

Given the following reaction at equilibrium, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) At constant pressure if some inert gas is added to the system. Then :<\/a><\/p>\n

For the reaction N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) ; \u0394H = \u2212 93 .6 kJmol \u2212 1 the number of moles of H 2 , at equilibrium will increase if :<\/a><\/p>\n

For which of the following reactions is product formation favoured by low pressure and high temperature?<\/a><\/p>\n

Favourable conditions for melting of ice is<\/a><\/p>\n

What is the correct relationship between free energy change and equilibrium constant of a reaction?<\/a><\/p>\n

van’t Hoffs equation shows the effect of temperature on equilibrium constants K c and K p the K p varies with temperature according to the relation<\/a><\/p>\n

The standard free energy change of a reaction is \u0394G \u00b0 = – 115 kJ at 298 K . Calculate the value of log 10 K p R = 8 . 314 JK – 1 mol – 1<\/a><\/p>\n

What is the unit of K p of the reaction? CS 2 ( g ) + 4 H 2 ( g ) \u21cc CH 4 ( g ) + 2 H 2 S ( g )<\/a><\/p>\n

Which one of the following conditions will favour maximum formation of the product in the reaction A 2 ( g ) + B 2 ( g ) \u21cc X 2 ( g ) , \u0394 r H = – X kJ ?<\/a><\/p>\n

For the reversible reaction N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) + heat The equilibrium shifts in forward direction<\/a><\/p>\n

2 B g \u21cc 3 C l + D g + 90 kJ , Favourable conditions for the formation of \u2018B\u2019 according to Lechatelier’s principle are<\/a><\/p>\n

A \u21cc 2 B ; K = 80 C \u21cc B ; K = 2 2 C \u21cc D ; K = 10 Equilibrium constant for the reaction A \u21cc D will be<\/a><\/p>\n

Which of the following neither effects equilibrium state nor efffects equilibrium constant<\/a><\/p>\n

For the process A g + 3 B g \u21cc 2 C g at 750 K the value of equilibrium constant is 10 2 . At 450K the value of equilibrium constant for the same reaction is 5 \u00d7 10 2 . Correct statement about the process is<\/a><\/p>\n

For a reversible reaction temperature is increased, the incorrect statement is<\/a><\/p>\n

Statement I: Addition of inertgas has no effect on equilibrium state when carried out at constant volume. Statement II: Molybdenum is the catalyst used in Haber’s process<\/a><\/p>\n

If the equilibrium constant for N 2 ( g ) + O 2 ( g ) \u21cc 2 NO ( g ) is K, the equilibrium constant for 1 2 N 2 ( g ) + 1 2 O 2 ( g ) \u21cc NO ( g ) will be<\/a><\/p>\n

At 298 K, K P < K C for the reaction<\/a><\/p>\n

Boyle’s temperature of four gases A, B, C, D are 100 K, 120 K, 140 K and 160 K respectively. At 150 K, positive deviations from ideal behaviour are observed in<\/a><\/p>\n

Hydrolysis of sucrose is given by the following reaction Sucrose + H 2 O \u21cc Glucose + Fructose If the equilibrium constant ( K C ) is 2 x 10 13 at 300 K, the value \u0394 r G \u0398 at the same temperature will be<\/a><\/p>\n

The equilibrium constants of the following are<\/a><\/p>\n

Which one of the following statements is not correct?<\/a><\/p>\n

The standard equilibrium constant, K p at 298 K for the reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 N H 3 ( g ) i s 5 . 8 x 10 5 . The value of standard equilibrium constant, if the concentration of gases is expressed in terms of mol\/L, will be: [Given: R = 0.08314 L bar K – 1 mol – 1 ]<\/a><\/p>\n

Consider the following reaction for which the change in enthalpy is positive. 2 A ( g ) + B ( g ) \u21cc C ( g ) + D ( g ) Which of the following will not affect the equilibrium?<\/a><\/p>\n

For the reaction CO ( g ) + Cl 2 ( g ) \u21cc COCl 2 ( g ) K p K c is equal to :<\/a><\/p>\n

COLUMN-I COLUMN-II (I) Q C \u2009\u2009\u2009 > \u2009\u2009\u2009 K C (a) Forward reaction is favoured (II) Q C \u2009\u2009\u2009 < \u2009\u2009\u2009 K C (b) Both forward and backward reactions are favoured (III) Q C \u2009\u2009\u2009 = \u2009\u2009\u2009 K C (c) Backward reaction is favoured Correct match is<\/a><\/p>\n

Column I Column II (a) PCl 5 g \u2009 \u21cc PCl 3 g + Cl 2 g (i) K p \u2009 < \u2009 K c (b) H 2 g + I 2 g \u2009 \u21cc \u2009 2 HI g (ii) K p \u2009 > \u2009 K c (c) N 2 g + 3 H 2 g \u2009 \u21cc 2 NH 3 g (iii) K p \u2009 = \u2009 K c Correct match is (a) (b) (c) 1 i ii iii 2 i iii ii 3 ii iii i 4 iii i ii<\/a><\/p>\n

Consider the following reversible reactions. In which of the following reaction, negligible amount of product is formed<\/a><\/p>\n

Consider the reversible reaction, A g \u2009 \u21cc \u2009 B g + C g . Initially two moles of \u2018A\u2019 is taken in a two litre vessel. Total moles at equilibrium were found to be three. Percentage of decomposition of A(g) is<\/a><\/p>\n

Law of mass action is applicable to<\/a><\/p>\n

Consider the reversible reaction, PCl 5 g \u21cc PCl 3 g + Cl 2 g ; According to Lechatelier’s principle,decomposition of PCl 5 is favoured at<\/a><\/p>\n

What will be the value of \u0394G 0 for the process at 298 K if the equilibrium constant for the process is 9 \u2009\u2009 \u00d7 \u2009\u2009\u2009 10 12<\/a><\/p>\n

Consider the reversible reaction, N 2 O 4 g \u21cc 2 NO 2 g ; At equilibrium, number of moles of reactants is equal to that of products. Degree of decomposition of N 2 O 4 is<\/a><\/p>\n

Consider the reversible reaction, AB s \u21cc A g + B g ; K p = 81 atm 2 , Equilibrium pressure would be<\/a><\/p>\n

Statement I ; Catalyst in Haber’s process is Molybdenum Statement II ; At equilibrium state, number of moles of reactants and products are always equal<\/a><\/p>\n

In the case of , CaCO 3 s \u21cc CaO s + CO 2 g , attainment of equilibrium state is noticed with the help of constancy in<\/a><\/p>\n

At low temperature, Nitrogen dioxide, a reddish brown gas gets associated to form the colourless dinitrogen tetroxide as in the reaction . Then at equilibirium<\/a><\/p>\n

Which of the following is correct for .<\/a><\/p>\n

Which of the following is a characteristic property of equilibrium?<\/a><\/p>\n

When a system, A g \u21cc B g , is in equilibrium state, true statement is<\/a><\/p>\n

An example of an irreversible reaction is<\/a><\/p>\n

Attainment of equilibrium can be noticed with the help of constancy of which of the following physical properties ?<\/a><\/p>\n

Which of the following is not a general characteristic of equilibria involving physical processes?<\/a><\/p>\n

Irreversible reaction among the following is<\/a><\/p>\n

Law of mass action is not applicable to C graphite \u21cc C diamond , because<\/a><\/p>\n

The reaction CaCO 3 \u21cc CaO +CO 2 in a lime kiln goes to completion because<\/a><\/p>\n

According to law of mass action, for CaCO 3 \u21cc CaO + CO 2 (R f = Rate of forward and R b = Rate of backward reactions)<\/a><\/p>\n

Units of K C for xA g \u21cc yB g is lit 2 mol -2 , then the values of x and y cannot be<\/a><\/p>\n

As per law of mass action, for the reaction, NH 4 HS s \u21cc NH 3 g + H 2 S g , ratio of rate constants of forward reaction to rate constant of backward reaction at equilibrium equals to<\/a><\/p>\n

The units of equilibrium constant K c for the following system is<\/a><\/p>\n

The ionisation constant of H 2 CO 3 as an acid in aqueous solution at room temperature is X. If the first and second ionisation constants of H 2 CO 3 are X 1 and X 2 respectively then<\/a><\/p>\n

In which of the following cases, does the reaction go nearer to completion ?<\/a><\/p>\n

If K 1 and K 2 are the equilibrium constants of equilibria A and B respectively, then the relationship between the two constants is<\/a><\/p>\n

What is the equilibrium expression for the reaction, ?<\/a><\/p>\n

The equilibrium constants for the stepwise formation of MCl, MCl 2 and MCl 3 are a, b and c respectively. If the equilibrium constant of formation of MCl 3 is K, which of the following is correct?<\/a><\/p>\n

K 1 and K 2 are the equilibrium constants for the following equilibria respectively K 1 and K 2 are related as :<\/a><\/p>\n

How much PCl 5 must be added to a one litre vessel kept at 250 0 C in order to obtain 0.1 mole of Cl 2 gas. K C for PCl 5 g \u21cc PCl 3 g + Cl 2 g is 0.0414 mol\/L<\/a><\/p>\n

PCl 5 dissociates as follows in a closed reaction vessel . If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl 5 is x, the partial pressure of PCl 3 will be<\/a><\/p>\n

Units of K p for the reaction, NH 4 COONH 2 s \u21cc 2 NH 3 g + CO 2 g , are<\/a><\/p>\n

The relationship between K p and K c is given by<\/a><\/p>\n

We know that the relationship between K C and K p is . What would be the value of for the reaction?<\/a><\/p>\n

For a reaction if K p > K c the forward reaction is favoured by<\/a><\/p>\n

For the equilibrium reaction, the relation between K p and K c is<\/a><\/p>\n

For the reaction , the K p \/K c is equal to<\/a><\/p>\n

In which of the following reaction K p and K c are equal<\/a><\/p>\n

For which of the following reactions, K p (RT) 2 = K c<\/a><\/p>\n

The following are some statements about units of K c and K p. A) K p has always units. B) K c has no units at all times. C) If \u0394n = o, then K p and K c have no units. The correct set is<\/a><\/p>\n

In the equilibrium The forward reaction can be favoured by<\/a><\/p>\n

What is the effect of a ten-fold increase in pressure on K p in the reaction at equilibrium<\/a><\/p>\n

In the dissociation of CaCO 3 in a closed vessel, the forward reaction is favoured by<\/a><\/p>\n

In a reversible reaction K c > K p and \u2206 H = + 40 K.Cal. The product will be obtained in less amount on<\/a><\/p>\n

If some HCl gas is passed into the reaction mixture at the equilibrium of this reaction,<\/a><\/p>\n

K c value of a gaseous reversible reaction is 5 mole \/ lit. If the pressure is increased for this system at equilibrium then<\/a><\/p>\n

Le chatelier's principle is applicable to<\/a><\/p>\n

For a reversible reaction K p < K c , for this reaction at equilibrium, increase of pressure favours<\/a><\/p>\n

If CO 2 is made to escape from the system then for the system<\/a><\/p>\n

In the reversible reaction the concentration of fluoride ions was made halved, then equilibrium concentration of Ca +2<\/a><\/p>\n

Consider the reaction equilibrium, On the basis of Le Chatelier's principle, the condition favourable for the forward reaction is<\/a><\/p>\n

Consider the gaseous reaction, A + B \u21cc 2 C + D + q kJ , favourable conditions for the formation of \u2018C\u2019 and \u2018D\u2019 according to Lechatelier’s principle are<\/a><\/p>\n

For the reaction the forward reaction at constant temperature is favoured by<\/a><\/p>\n

The solubility of CO 2 in water increases with<\/a><\/p>\n

Solubility of a substance which dissolves with decrease in volume and absorption of heat will be favoured by<\/a><\/p>\n

Consider the equilibrium PCl 5(g) \u21cc PCl 3(g) + Cl 2(g) in a closed container. At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements holds true regarding the equilibrium constant (K p ) and degree of dissociation( \u03b1 )?<\/a><\/p>\n

In the case of gaseous homogeneous reaction, the active mass of the reactant is obtained by the expression<\/a><\/p>\n

Under what conditions of temperature and pressure the formation of atomic hydrogen from molecular hydrogen is favoured?<\/a><\/p>\n

High temperature and high pressure (as per Lechatelier principle) favour<\/a><\/p>\n

Favourable conditions for getting good yield of diamond (density of graphite and diamond are 2.3 g\/ml, 3.5 g\/ml).<\/a><\/p>\n

As per Braun's principle, yield of Ammonia will be more in Haber's process under ….. conditions (L=Low ; H = High, T = Temperature, P = Pressure)<\/a><\/p>\n

For at equilibrium, to shift equilibrium towards right,<\/a><\/p>\n

When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture it becomes pink. On the basis of this information mark the correct answer.<\/a><\/p>\n

\\ Rise of temperature shifts equilibrium towards right in the case of<\/a><\/p>\n

For the reaction PCl 3 + Cl 2 \u21cc PCl 5 the position of equilibrium can be shifted to the right by<\/a><\/p>\n

K C for at 500 K is , now backward reaction is favoured by<\/a><\/p>\n

For a dibasic acid, H 2 A \u21cc HA – + H + K 1 HA – \u21cc A 2 – + H + K 2 H 2 A \u21cc 2 H + + A 2 – ( K ) then<\/a><\/p>\n

Which of the following does not affect the degree of ionisation ?<\/a><\/p>\n

In the reaction, CaCO 3 s \u21cc CaO s + CO 2 g , 50 grams of CaCO 3 is allowed to dissociate in 22.4 lit vessel at 819 0 c . If 50% of CaCO 3 is left at equilibrium, active masses of CaCO 3 , CaO and CO 2 at equilibrium respectively are<\/a><\/p>\n

What is the equation for the equilibrium constant (K C ) for the following reaction ?<\/a><\/p>\n

For the equilibrium K p = 0.82 atm at 27 0 C. At the same temperature its K c in mol lit -1 is (R = 0.082 lit atm mol -1 K -1 )<\/a><\/p>\n

The compounds A and B are mixed in equimolar proportion to form the products, . At equilibrium 1 3 rd of each A and B reacted. Equilibrium constant for the reaction is<\/a><\/p>\n

One mole of A (g) is heated to 300 0 C in a closed one litre vessel till the following equilibrium is reached. The equilibrium constant of the reaction at 300 0 C is 4. What is the conc. of B (in, mole. lit -1 ) at equilibrium ?<\/a><\/p>\n

For the hypothetical reactions, the equilibrium constant (K) values are given K 1 = 2.0; K 2 = 4.0 K 3 = 3.0 The equilibrium constant for the reaction is<\/a><\/p>\n

The gaseous reaction, N 2 + 3 H 2 \u21cc 2 NH 3 , takes place at 450 0 c . 1 mole of Nitrogen and 2 mole of Hydrogen are mixed in a 1 litre vessel and 1 mole of Ammonia is formed at equilibrium. Then K c for the above reaction is<\/a><\/p>\n

In the reaction , the initial concentration of B is two times that of 'A'. But equilibrium concentration of B & C were found to be equal. Then the K C for the above system is<\/a><\/p>\n

The reversible reaction takes place in two reversible steps (2 and 3) with equilibrium constant values 2.0 and 0.45 respectively The equilibrium constant K c for the reaction (1) is<\/a><\/p>\n

2 mole of PCl 5 is heated in a one litre vessel. If PCl 5 dissociates to the extent of 80%, the equilibrium constant for the dissociation of PCl 5 is<\/a><\/p>\n

28 gms of N 2 and 6 gms of H 2 were heated in a closed 1litre vessel. At equilibrium, 25.5 gms of NH 3 is present. The approximate value of K C is<\/a><\/p>\n

The K C for the reaction I 2(g) \u21cc 2I (g) is 4 \u00d7 10 -3 . If the equilibrium concentration of atomic iodine is 4 \u00d7 10 -2 M . What is the concentration of molecular iodine ?<\/a><\/p>\n

In a 500 ml flask, the degree of dissociation of PCl 5 at equilibrium is 40% when the initial amount taken is 5 moles. The value of equilibrium constant in moles\/lit for the decomposition of PCl 5 is ( Given reaction, PCl 5 g \u21cc PCl 3 g + Cl 2 g )<\/a><\/p>\n

One mole of A (g) is heated to 200 0 C in a 1 lit closed flask, till the following equilibrium is reached A (g) \u21cc B (g) . The rate of forward reaction at equilibrium is 0.02 mole.lit -1 .min -1 . What is the rate (in mole.lit -1 .min -1 ) of the backward reaction at equilibrium ?<\/a><\/p>\n

At 298K, the molar equilibrium concentrations of Ag + , NH 3 and [Ag(NH 3 ) 2 ] + for the equilibrium Ag + (aq) + 2NH 3(aq) \u21cc [Ag(NH 3 ) 2 ] + (aq) were found to be 10 -1 , 10 -3 , and 10 -1 respectively. The value K c is<\/a><\/p>\n

At 298K, the molar equilibrium concentrations of Ag + , NH 3 and [Ag(NH 3 ) 2 ] + for the equilibrium Ag aq + + 2 NH 3 aq \u21cc Ag NH 3 2 aq + were found to be 10 -1 , 10 -3 , and 10 -1 respectively. The value K c is<\/a><\/p>\n

At certain temperature, a 10 lit vessel contains 0.4 mole H 2 , 0.4 mole I 2 & 0.1 mole HI at equilibrium. Then K p for is<\/a><\/p>\n

3 mole of reactant A and one mole of reactant B are mixed in a vessel of volume 1 litre. The reaction taking place is . If 1.5 mol of C is formed at equilibrium, the value of K c is<\/a><\/p>\n

In the process (in aq medium), initially there are 2 mole I 2 & 2 mole I – . But at equilibrium, due to addition of AgNO 3(aq) , 1.75 mole yellow ppt is obtained. K C for the process is (V flask =1 dm 3 ) nearly<\/a><\/p>\n

At constant temperature & volume, 50% of ozone is decomposed out of 2 atm of ozone taken initially and the equilibrium is established, Kp for the decomposition of ozone is<\/a><\/p>\n

For the reaction , the partial pressures of CO 2 and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the value of K p for this reaction?<\/a><\/p>\n

1 mole CaCO 3(s) is heated in 11.2 lit vessel so that equilibrium is established at 819 K. If K P for at this temperature is 2 atm, equilibrium concentration of CO 2 (in mol-lit -1 )<\/a><\/p>\n

In the reaction is 50% dissociated at 27 0 C when the equilibrium pressure is 0.5 atm. Partial pressure of SO 3(g) at Equilibrium is<\/a><\/p>\n

For , equilibrium pressure at 2000K is 100 atm. Now, K P for the process is (in atm 2 )<\/a><\/p>\n

At 227 0 C and 4 atm, PCl 5 is dissociated to an extent 50%. At same temperature, extent of dissociation of PCl 5 is 0.75 at a pressure of<\/a><\/p>\n

For the reaction , the degree of dissociation at equilibrium is 0.2 at 1 atm. Then K p will be<\/a><\/p>\n

At a certain temperature, the degree of dissociation of PCl 5 was found to be 0.25 under a total pressure of 15 atm. The value of K p for the dissociation of PCl 5 in the reaction, PCl 5 g \u21cc PCl 3 g + Cl 2 g<\/a><\/p>\n

AB 2 dissociates as : When the intial pressure of AB 2 is 500 mm Hg, the total equilibrium pressure is 700 mm Hg. Calculate equilibrium constant for the reaction, assuming that the volume of the system remains unchanged.<\/a><\/p>\n

For the reversible reaction at 500 0 C. The value of K p is 1.44×10 -5 , when partial pressure is measured in atmospheres. The corresponding value of K c with concentration in mol L -1 is<\/a><\/p>\n

K C for at certain temperature is 1.6 × 10 -3 , then K P for at same temperature will be<\/a><\/p>\n

The value of Kp for the reaction is 1.2 × 10 -2 at 1065 0 C. The value of Kc for this reaction is<\/a><\/p>\n

K P \/ K C for (gaseous phase) at 400 K is<\/a><\/p>\n

For , initially 1 mole each of XY 2 & Y are present in 10 lit flask at 500 mm. If the equilibrium pressure of XY is 150mm, K P is<\/a><\/p>\n

For , at equilibrium . Then, temperature at which K P = 1 ?<\/a><\/p>\n

Vapour density of PCl 5 is 104.16 but when heated to 230 o C its vapour density is reduced to 62. The degree of dissociation of PCl 5 at this temperature will be<\/a><\/p>\n

Statement I : Effect of temperature on K C or K P depends on enthalpy change. Statement II : Increase in temperature shifts the equilibrium in exothermic direction & decrease in temperature shifts the equilibrium in endothermic direction.<\/a><\/p>\n

Statement I : The degree of decomposition of PCl 5 is more at low pressures. Statement II : In a reversible reaction, on increasing the pressure the equilibrium shifts in the direction in which decrease in volume takes place.<\/a><\/p>\n

Statement I : The active mass of a pure solid or a pure liquid is taken as unity. Statement II : The active mass of a pure solid or liquid depends on density which is constant for a pure substance.<\/a><\/p>\n

Statement I : If pressure is increased on ice water equilibrium, more water will change into ice. Statement II : Melting of solids is generally accompanied by increase in volume, hence increase of pressure shifts the equilibrium in the direction in which volume increases.<\/a><\/p>\n

The decomposition of N 2 O 4 to NO 2 is carried out at 280K in chloroform. When equilibrium has been established, 0.2 mole of N 2 O 4 and 2 \u00d7 10 \u20133 mole of NO 2 are present in 2 litre solution. The equilibrium constant for reaction N 2 O 4 \u21cc 2 NO 2 is<\/a><\/p>\n

For the chemical equilibrium can be determined from which one of the following plots<\/a><\/p>\n

The standard state Gibbs free energy change for the given isomerization reaction Cis – 2 -Pentene \u21cc trans – 2- pentene is -3.67kJ\/mol at 400K. If more trans-2-pentene is added to the reaction vessel, then<\/a><\/p>\n

The dissociation equilibrium of a gas AB 2 can be represented as The degree of dissociation is x and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant Kp and total pressure p is<\/a><\/p>\n

Two solids dissociate as follows The total pressure when both the solids dissociate simultaneously is<\/a><\/p>\n

At 700K, the equilibrium constant K P for the reaction 2SO 3(g) \u21cc 2SO 2(g) + O 2(g) is 1.80 \u00d7 10 \u20133 , (R = 8.314 JK \u20131 mole \u20131 ). The numerical value in moles per lit of K C for this reaction at the same temperature will be<\/a><\/p>\n

For the reaction. H 2 + I 2 \u21cc 2 HI, K = 47.6. If the intial number of moles of each reactant and product is 1mole then at equilibrium<\/a><\/p>\n

Kp for the reaction A \u21cc B is 4. If initially only A is present then what will be the partial pressure of B after equilibrium ?<\/a><\/p>\n

For the reaction the correct relation is<\/a><\/p>\n

In the reaction 2SO 2(g) + O 2(g) \u21cc 2SO 3(g) , 2 moles of SO 2 ,1 mole of O 2 and 2 moles of SO 3 are present in equilibrium. what is the number of moles of O 2 be introduced into the vessel to increase the equilibrium moles of SO 3 to 3 moles<\/a><\/p>\n

The vapour density of undecomposed N 2 O 4 is 46. When heated, vapour density decreases to 24.5 at equilibrium due to its dissociation to NO 2 . The percent dissociation of N 2 O 4 at equilibrium is equal to<\/a><\/p>\n

The rate constant for forward reaction is two times of rate constant for backward reaction at a given temperature. Then K c will be<\/a><\/p>\n

The degree of dissociation of PCl 5 obeying the equilibrium , is approximately related to the pressure at equilibrium by<\/a><\/p>\n

Based on Lechatelier’s principle, false statement among the following is<\/a><\/p>\n

For the reversible reaction, X 2 g \u21cb 2 X g carried out in a one litre closed vessel, the number of moles of reactants and products at equilibrium are equal. Degree of decomposition of X 2 g is<\/a><\/p>\n

When ice and water are kept in perfectly insulated thermos flask at 273 K and 1 atmosphere, which of the following is not correct?<\/a><\/p>\n

The following graph does not represent for A + B \u21cc C + D ?<\/a><\/p>\n

Two separate chamber containing equilibrium mixtures of H 2 , N 2 , NH 3 and D 2 , N 2 , ND 3 are connected with each other. After some time the mixture will contain<\/a><\/p>\n

Which of the following facts are correct for the plot shown below for H 2 ( g ) + I 2 ( g ) \u21cc 2 HI ( g ) ?<\/a><\/p>\n

At equilibrium, the concentrations of N 2 = 3 . 0 \u00d7 10 – 3 M , O 2 = 4 . 2 \u00d7 10 – 3 M and NO = 2 . 8 \u00d7 10 – 3 M in a sealed vessel at 800 K. What will be K C for the reaction N 2 g + O 2 g \u21cc 2 NO g ?<\/a><\/p>\n

Equilibrium constant of H 2 g + I 2 g \u21cc 2HI(g) is 2 \u00d7 10 – 4 . What is the equilibrium concentration of HI, if concentrations of and H 2 g I 2 g respectively are 2 . 2 \u00d7 10 – 2 M and 2 . 2 \u00d7 10 – 4 M ?<\/a><\/p>\n

The equilibrium system in which all reactants and products are in the same phase is called as<\/a><\/p>\n

K C for the following equilibrium (I) is 2 . 0 \u00d7 10 – 4 under certain condition, the equilibrium constant of (II) is (I) H 2 g + I 2 g \u21cc 2 HI (II) 2 H 2 g + 2 I 2 g \u21cc 4 HI<\/a><\/p>\n

Which of the following represents homogeneous equilibrium?<\/a><\/p>\n

For a homogeneous gaseous equilibrium, which of the following is correct?<\/a><\/p>\n

Equilibrium state in system that contains more than one phase of reactants and products is called<\/a><\/p>\n

Which of the following equilibrium constant expression is not correct?<\/a><\/p>\n

Select the correct choice for the following rules I, II and III. At equilibrium: I. K c > 10 3 \u21d2 Products are negligible II. K c < 10 – 3 \u21d2 Reactants are negligible III. 10 – 3 < K c < 10 3 \u21d2 Reactants and products both are present in considerable quantitites.<\/a><\/p>\n

Out of the following, which reaction has both reactants and products in considerable quantities at equilibrium.<\/a><\/p>\n

For the reversible reaction aA + bB \u21cc cC+dD which of the following is\/are correct?<\/a><\/p>\n

The values of K p 1 and K p 2 for the reactions X \u21cc Y + Z (i) and A \u21cc 2 B (ii) are in the ratio of 9 : 1. If the degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and (ii) are in the ratio<\/a><\/p>\n

The dissociation equilibrium of a gas AB 2 can be represented as 2 AB 2 g \u21cc 2 AB ( g ) + B 2 ( g ) The degree of dissociation is x and is small compared to 1. The expression relating to the degree of dissociation (x) with equilibrium constant K p and total pressure P is<\/a><\/p>\n

Consider the following gaseous reversible reactions occuring in a closed vessel. Addition of argon gas at constant pressure favours forward reaction in the case of<\/a><\/p>\n

For the process, A g \u21cc B g + C g the value of K p in terms of degree of decomposition \u03b1 of \u2018A\u2019 and equilibrium pressure (P) is<\/a><\/p>\n

Column-I Column-II (p) aA + bB \u21cc cC + dD (i) K c ‘ = 1 K c (q) cC + dD \u21cc aA + bB (ii) K c ” = K c n (r) naA + bB \u21cc ncC + dD (iii) K c<\/a><\/p>\n

Statement-I: On addition AB + C \u21cc AC + B ; AC + D \u21cc AD + C ; AB + D \u21cc AD + B ; K net = K 1 \u00d7 K 2 Eqm. constt.= K 1 Eqm. constt.= K 2 Eqm. constt.= K net Statement-II: the equilibrium constant K net for a net reaction obtained by adding two or more reactions is equal to the product of equilibrium constants for individual reactions.<\/a><\/p>\n

Statement-I: For the reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) Unit of K c = L 2 mol – 2 Statement-II: For the reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) Eqm . constant , K c = [ NH 3 ] 2 [ N 2 ] [ H 2 ] 3<\/a><\/p>\n

Statement-I: A catalyst can start and speed up all reactions. Statement-II: The value of equilibrium constant is not affected by a catalyst.<\/a><\/p>\n

Statement-I: For a gaseous reaction, aA + bB \u21cc cC + dD , K p = K c Statement-II: Concentrations of solid substances are taken unity.<\/a><\/p>\n

We know that the relationship between K c and K p is K p = K c RT \u2206 n What would be the value of \u2206 n for the reaction NH 4 Cl s \u21cc NH 3 g + HCl g ?<\/a><\/p>\n

PCl 5 , PCl 3 and Cl 2 are at equilibrium at 500 K in a closed container and their concentrations are 0 . 8 \u00d7 10 – 3 mol L – 1 , 1 . 2 \u00d7 10 – 3 mol L – 1 and 1 . 2 \u00d7 10 – 3 mol L – 1 respectively. The value of K c for the reaction PCl 5 g \u21cc PCl 3 g + Cl 2 g will be<\/a><\/p>\n

The temperature at which magnitude of K p units = atm \u2206 n and K c units = mole \/ lit \u2206 n are always equal for every gaseous reaction is<\/a><\/p>\n

Which one of the following is an example of heterogeneous equilibrium<\/a><\/p>\n

Consider the gaseous reversible reaction, A + 2 B \u21cc 2 C + D occuring in a one litre closed vessel. Initially 1 mole of \u2018A\u2019 and 2 moles of \u2018B\u2019 are taken. At equilibrium 1 mole of \u2018C\u2019 is formed. Value of equilibrium constant K c is<\/a><\/p>\n

For the reaction, PCl 5 ( g ) \u21cc PCl 3 ( g ) + Cl 2 ( g ) at 121.8K . logK p – logK c is equal to (R = 0.0821 lit atm K -1 mole -1 )<\/a><\/p>\n

For the reversible reaction, A s \u21cc B s + C g ; \u2206 H = + 180 kJ , forward reaction is favoured<\/a><\/p>\n

A hypothetical gaseous reversible reaction A g \u21cc B g + C g is carried out at 9 Kelvin. The correct relation between K p and K c is (Units of K p are \u2018atm\u2019 and K c are \u2018mole\/lit\u2019)<\/a><\/p>\n

Statement-I : Addition of \u2018Ar\u2019 gas at constant volume favours the decomposition of PCl 5 (g) Statement-II : In a reversible reaction, addition of catalyst favours forward reaction only.<\/a><\/p>\n

Which one of the following statements is correct?<\/a><\/p>\n

Which of the following is incorrect regarding equilibrium state?<\/a><\/p>\n

Which of the following statements is correct regarding liquid vapour equilibrium state at a given temperature?<\/a><\/p>\n

Ice and water kept in a perfectly insulated thermos flask at 273K and atmospheric pressure ,are in equilibrium state then the system shows<\/a><\/p>\n

In an experiment, if we expose three watch glasses containing separately 1 mL each of acetone, ethyl alcohol and water to atmosphere and repeat the experiment with different volumes of the liquids in a warmer room. It is observed that in all such cases the liquid eventually disappears and the time taken for complete evaporation depends on<\/a><\/p>\n

For any pure liquid at 1atm pressure (1.013 bar), the temperature at which the liquid and vapours are at equilibrium is called<\/a><\/p>\n

Which of the following statements is correct?<\/a><\/p>\n

When both forward and backward reactions occur at the same rate, the system reaches<\/a><\/p>\n

A mixture of reactants and products in the equilibrium state is called<\/a><\/p>\n

A pressure change obtained by changing the volume can affect the yield of products in case of a gaseous reaction, where<\/a><\/p>\n

Which one of the following informations can be obtained on the basis of Le-Chatelier principle?<\/a><\/p>\n

The degree of ionisation of a compound depends on<\/a><\/p>\n

While comparing, the ionisation of hydrochloric acid with that of acetic acid in water we find that though both of them are polar covalent molecules, former is completely ionised into its constituent ions, while the latter is only partially ionised (< 5%). The reason is that<\/a><\/p>\n

The solutions which resist change in pH on dilution or with the addition of small amounts of acid or alkali are called<\/a><\/p>\n

A solution of an acid has pH = 4.70. Find out the concentration of OH – ions ( pK w =14).<\/a><\/p>\n

For a reaction, CH 3 COOH ( aq ) \u21cc H + ( aq ) + CH 3 COO – ( aq ) or HAc ( aq ) \u21cc H + ( aq ) + Ac – ( aq ) Evaluate the pH of the solution resulting on addition of 0.05 M acetate ion to 0.05 M acetic acid solution K a = 1 . 8 \u00d7 10 – 5<\/a><\/p>\n

The dissociation constant of water is represented by K = H 3 O + OH – \/ H 2 O or K w = H + OH – K w is called<\/a><\/p>\n

The solubility product ( K sp ) of solid barium sulphate at 298 K is 1 . 1 \u00d7 10 – 10 . The molar solubility, (S ) of Ba 2 + and SO 4 2 – are<\/a><\/p>\n

Calculate the molar solubility (S) of a salt like zirconium phosphate of molecular formula Zr 3 PO 4 4<\/a><\/p>\n

In the chemical reaction, N 2 + 3 H 2 \u21cc 2 NH 3 at equilibrium point,<\/a><\/p>\n

Which of the following is the example of a reversible reaction?<\/a><\/p>\n

The method of preparation of ammonia can be represented graphically as N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) In the above graph, X,Y and Z respectively are<\/a><\/p>\n

The active mass of 64 g of HI in a 2L flask would be<\/a><\/p>\n

For a reaction, H 2 ( g ) + I 2 ( g ) \u21cc 2 HI ( g ) K C = [ HI ] 2 H 2 I 2 Point out the correct statement.<\/a><\/p>\n

In the equilibrium, AB \u21cc A + B , if the equilibrium concentration of A is double, then equilibrium concentration of B will be<\/a><\/p>\n

K C for the reaction, N 2 ( g ) + O 2 ( g ) \u21cc 2 NO ( g ) at 300 K is 4 . 0 \u00d7 10 – 6 \u00b7 K p for the above reaction will be R = 2 calmol – 1 K – 1<\/a><\/p>\n

For the reversible reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) at 500 \u00b0 C , the value of K p is 1 . 44 \u00d7 10 – 5 , when the partial pressure is measured in atmospheres. The corresponding value of K C with concentration in molL – 1 is<\/a><\/p>\n

For the reaction, I 2 ( g ) \u21cc 2 I ( g ) ; K C = 37 . 6 \u00d7 10 – 6 at 1000 K. If 1.0 mole of I 2 ir introduced into a 1.0 L flask at 1000 K, at equilibrium<\/a><\/p>\n

For the reaction, SO 2 ( g ) + 1 2 O 2 ( g ) \u21cc SO 3 ( g ) if K p = K C ( RT ) x where, the symbols have usual meaning, then the value of x is (assuming ideality)<\/a><\/p>\n

For the equilibrium, 2 NOCl ( g ) \u21cc 2 NO ( g ) + Cl 2 ( g ) the value of the equilibrium constant, K C is 3 . 75 \u00d7 10 – 6 at 1069 K Calculate the K p for the reaction at this temperature.<\/a><\/p>\n

PCl 5 , PCl 3 and Cl 2 are at equilibrium at 500 K and having concentration 1 . 59 M PCl 3 , 1 . 59 M Cl 2 and 1 . 41 M PCl 5 Calculate K C for the reaction, PCl 5 \u21cc PCl 3 + Cl 2<\/a><\/p>\n

Consider the following equilibrium in a closed container, N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) . At a fixed temperature, the volume of the reaction container is halved. For this change which of the following statements hold true regarding the equilibrium constant ( K p ) and degree of dissociation ( \u03b1 )?<\/a><\/p>\n

Which of the following reactions show(s) heterogeneous equilibria?<\/a><\/p>\n

For CaCO 3 ( s ) \u21cc \u0394 CaO ( s ) + CO 2 ( g ) , the equilibrium constant K C and K p for the thermal decomposition of calcium carbonate is<\/a><\/p>\n

The equilibrium constants for the reaction, Zn ( s ) + Cu 2 + ( aq ) \u21cc Zn 2 + ( aq ) + Cu ( s ) and Cu ( s ) + 2 Ag + ( aq ) \u21cc Cu 2 + ( aq ) + 2 Ag ( s ) are K 1 and K 2 respectively. The equilibrium constant for the combined reaction is<\/a><\/p>\n

For the reaction, H 2 ( g ) + I 2 ( g ) \u21cc 2 HI ( g ) ; K C = 57 . 0 at 700 K . The molar concentration of H 2 = 0 . 10 M , I 2 = 0 . 20 M and [ HI ] = 0 . 40 M . Calculate the reaction quotient, Q C of the reaction.<\/a><\/p>\n

Which of the following equation represents the correct relationship between reaction quotient, Q and Gibbs energy, G?<\/a><\/p>\n

Using the equation ( K = e – \u0394G \u00b0 \/ RT ), the reaction spontaneity can be interpreted in terms of the value of \u0394G \u00b0 is\/are<\/a><\/p>\n

In which condition, the reaction proceeds in the forward direction?<\/a><\/p>\n

Production of ammonia according to the reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) \u0394H = – 92 . 3 \u2223 8 kJ mol – 1 is an exothermic process. At low temperature, the reaction shifts in<\/a><\/p>\n

For the reversible reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) + Heat The equilibrium shifts in forward direction<\/a><\/p>\n

Which one of the following informations can be obtained on the basis of Le-Chatelier principle?<\/a><\/p>\n

Ostwald’s process for the manufacfure of nitric acid involves the reaction, 4 NH 3 ( g ) + 5 O 2 ( g ) \u21cc 4 NO ( g ) + 6 H 2 O ( l ) \u0394H = + Q kJ Which of the following factors will not affect the concentration of NH 3 at equilibrium?<\/a><\/p>\n

Of the following, which change will shift the reaction towards the product at equilibrium? I 2 ( g ) \u21cc 2 I ( g ) ; \u0394H \u00b0 ( 298 K ) = + 150 kJ<\/a><\/p>\n

Dissolution of sodium sulphate is an exothermic process. If a saturated solution of sodium sulphate containing extra undissolved sodium sulphate is heated, then<\/a><\/p>\n

Consider the following statements regarding physical processes. I. Equilibrium is possible only in a closed system at a given temperature. II. Both the opposing processes occur at the same rate and there is a dynamic but stable condition. III. All measurable properties of the system remain constant. IV. When equilibrium is attained for a physical process, it is characterised by constant value of one of its parameters at a given temperature. V. The magnitude of such quantities at any stage indicates the extent to which the physical process has proceeded before reaching, equilibrium. Which of the following option is correct?<\/a><\/p>\n

Consider the following statements regarding the equilibrium constants. I. Expression for the equilibrium constant is not applicable when concentrations of the reactants and products have attained constant value at equilibrium state. II. The value of equilibrium constant is dependent on initial concentration of the reactants and products. III Equilibrium constant is temperature dependent having one unique value for a particular reaction represented by a balanced equation at a given temperature. IV. The equilibrium constant for the reverse reaction is directly proportional to the equilibrium constant for the forward reaction. Choose the correct statement(s) is\/are<\/a><\/p>\n

Statement I: The vapour pressure of gas on liquid is constant at a given temperature. Statement II: It is the state of liquid \u21cc vapour equilibrium<\/a><\/p>\n

Consider the following statement about the a equilibrium, 2 SO 2 ( g ) + O 2 ( g ) \u21cc 2 SO 3 ( g ) ; \u0394H \u00b0 = – 198 kJ I. On decreasing the temperature as well as pressure equilibrium shifts in forward direction. II. On increasing temperature and pressure equilibrium shifts in forward direction. III. On decreasing the temperature and increasing the pressure, equilibrium will shift in forward direction. Choose the correct option.<\/a><\/p>\n

Statement I: N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) is the example of homogeneous equilibria. Statement II: For this reaction, K C has unit L\/mol and K p has unit bar<\/a><\/p>\n

Statement I: The dynamic nature of chemical equilibrium can be demonstrated in the synthesis of ammonia by Haber’s process. Statement II: In a series of experiments, Haber started with known amounts of dinitrogen and dihydrogen maintained at high temperature and pressure and at regular intervals determined the amount of ammonia present and concentration of unreacted dihydrogen and dinitrogen.<\/a><\/p>\n

Statement I: For dissolution of solids in liquids, the solubility is constant at a given temperature. Statement II: For dissolution of gases in liquids, the concentration of a gas in liquid is inversely proportional to the pressure (concentration) of the gas over the liquid<\/a><\/p>\n

In the reaction A+B C+D, initial concentration of A and B both are equal. At equilibrium, the concentration of D is twice as that of A. What will be the equilibrium constant of the reaction?<\/a><\/p>\n

Statement I: In the equilibrium between nickel, carbon monoxide and nickel carbonyl which is used in the purification of nickel, represented as Ni ( s ) + 4 CO ( g ) \u21cc Ni ( CO ) 4 ( g ) Statement II: The equilibrium constant for a reaction is K C = Ni ( CO ) 4 [ CO ] 4<\/a><\/p>\n

Statement I: The equilibrium constant for a net reaction obtained after adding two (or more) reactions equals the product of the equilibrium constants for individual reactions. Statement II: The expression is K net = K 1 \u00d7 K 2 \u00d7 \u2026<\/a><\/p>\n

Statement I: If a volume is kept constant and an inert gas such as argon is added which does not take part in the reaction, the equilibrium remains undisturbed. Statement II: It is because the addition of an inert gas at constant volume does not change the partial pressure or the molar concentrations of the substance involved in the reaction.<\/a><\/p>\n

Statement I: Catalyst does not affect the equilibrium composition of a reaction mixture. Statement II: It does not appear in the balanced chemical equation or in the equilibrium constant expression.<\/a><\/p>\n

Statement I: Both the opposing processes in equilibrium reactions occur simultaneously. Statement II: The system is in dynamic equilibrium.<\/a><\/p>\n

Match the Column I with Column II and choose the correct option from the codes given below. Column I (Process) Column II (Conclusion) A. Liquid \u21cc vapour 1. Concentration of solute in solution is constant at a given temperature. B. Solid \u21cc liquild 2. [ Gas ( aq ) ] [ Gas ( s ) ] is – constant at a given temperature. C. Solute ( S ) \u21cc solute ( solution ) 3. P H 2 O constant at given temperature D. Gas ( g ) \u21cc Gas ( aq ) 4. Melting point is fixed at constant pressure. Codes<\/a><\/p>\n

Match the Column I with Column II and choose the correct option from the codes given below. Column I (Reaction) Column II ( K p ) A. N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 at 298 K 1. 2 . 5 \u00d7 10 10 B. 2 SO 2 + O 2 ( g ) \u21cc 2 SO 3 ( g ) at 500 K 2. 6 . 8 \u00d7 10 5 C. N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) at 400 K 3. 47.9 4. 3 . 6 \u00d7 10 – 2 Codes<\/a><\/p>\n

Match the Column I with Column II and choose the correct option from the codes given below. Column I (Process) Column II (Conclusion) A. Liquid \u21cc vapour 1. Concentration of solute in solution is constant at a given temperature. B. Solid \u21cc liquild 2. [ Gas ( aq ) ] [ Gas ( s ) ] is – constant at a given temperature. C. Solute ( S ) \u21cc solute ( solution ) 3. P H 2 O constant at given temperature D. Gas ( g ) \u21cc Gas ( aq ) 4. Melting point is fixed at constant pressure. Codes<\/a><\/p>\n

A vessel at 1000 K contains CO 2 with a pressure of 0.5 atm. Some of CO 2 is converted into CO on addition of graphite. The value of K at 1000 K, when total pressure equilibrium is 0.8atm will be<\/a><\/p>\n

For the following equilibrium, N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) K p is found to be equal to K C . This is attained when<\/a><\/p>\n

When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture it becomes pink. On the basis of this information mark the correct answer Co H 2 O 6 3 + (Pink ) ( aq ) + 4 Cl – ( aq ) \u21cc CoCl 4 2 – (Blue) ( aq ) + 6 H 2 O ( l )<\/a><\/p>\n

For the reaction, H 2 ( g ) + I 2 ( g ) \u21cc 2 HI ( g ) , the standard free energy is \u0394G \u00b0 > 0 . The equilibrium constant ( K C ) would be<\/a><\/p>\n

On increasing the pressure, in which direction will the gas phase reaction proceed to re-establish equilibrium, is predicted by applying the Le-Chatelier’ s principle. Consider the reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) Which of the following is correct, if the total pressure at which the equilibrium is established, is increased without changing the temperature?<\/a><\/p>\n

Identify correct statements among the following A) A catalyst can influence equilibrium state B) At equilibrium, \u2206 G is always zero C) Law of mass action is applicable to physical process only D) When Q c > K c , backward reaction is favoured<\/a><\/p>\n

Identify correct statements among the following A) A catalyst cannot influence equilibrium state B) At equilibrium, \u2206 o G is always zero C) Law of mass action is applicable to physical process only D) When Q c > K c , backward reaction is favoured<\/a><\/p>\n

Molecular hydrogen is obtained from gaseous hydrogen atoms. Favourable conditions for the formation of hydrogen atoms from hydrogen molecule according to Leachatelier’s principle are<\/a><\/p>\n

Consider a reversible reaction taking place in a 10 litre closed vessel at 300K, X g \u21cc 2 Z g ; Initially two moles of \u2018X\u2019 is present in the vessel. At equilibrium two moles of \u2018Z\u2019 is formed. K c for the reaction at 300 K will be<\/a><\/p>\n

Consider a reversible reaction taking place in a 10 litre closed vessel at 300K, X g \u21cc 2 Z g ; Initially two moles of \u2018X\u2019 is present in the vessel. At equilibrium two moles of \u2018Z\u2019 is formed. K c for the reaction at 300 K will be<\/a><\/p>\n

Consider the reversible reaction, X 2 g \u21cc 2 X g ; At equilibrium, number of moles of reactants is equal to that of products. Degree of decomposition of X 2 is<\/a><\/p>\n

Statement I ; Catalyst in Haber’s process is Platinised asbestos Statement II ; At equilibrium state, number of moles of reactants and products are always equal<\/a><\/p>\n

Consider the reversible reaction, A g \u21cc B g + C g ; K c = 1 M at 300K. Value of K p at the same temperature is<\/a><\/p>\n

Consider the reversible reaction, AB s \u21cc A g + B g ; K p = 9 atm 2 , Equilibrium pressure would be<\/a><\/p>\n

A reversible reaction is one which<\/a><\/p>\n

The equilibrium constant K c for the reaction P 4 ( g ) \u21cc 2 P 2 ( g ) is 1.4 at 400 o c. Suppose that 3 moles of P 4 (g) and 2 moles of P 2 (g) are mixed in 2 liter container at 400 o c. What is the value of reaction quotient (Q c )?<\/a><\/p>\n

In a chemical reaction equilibrium is established when<\/a><\/p>\n

For the reaction A ( g ) + 3 B ( g ) \u21cc 2 C ( g ) at 27 \u00b0 C , 2 moles of A, 4 moles of B and 6 moles of C are present in 2 litre vessel. If K c for the reaction is 1.2, the reaction will proceed in :<\/a><\/p>\n

For a reversible gaseous reaction N 2 + 3 H 2 \u21cc 2 NH 3 at equilibrium, if some moles of H 2 are replaced by same number of moles of T 2 (T is tritium, isotope of H and assume isotopes do not have different chemical properties) without affecting other parameters, then :<\/a><\/p>\n

For the synthesis of ammonia by the reaction N 2 + 3 H 2 \u21cc 2 NH 3 in the Haber’s process, the attainment of equilibrium is correctly predicted by the curve<\/a><\/p>\n

Attainment of the equilibrium A ( g ) \u21cc 2 C ( g ) + B ( g ) gave the following graph. Find the correct option.(% dissociation = fraction dissociated x 100)<\/a><\/p>\n

What is the equilibrium expression for the reaction P 4 ( s ) + 5 O 2 ( g ) \u21cc P 4 O 10 ( s )<\/a><\/p>\n

. At 527 o c, the reaction given below has K c =4 NH 3 ( g ) \u21cc 1 2 N 2 ( g ) + 3 2 H 2 ( g ) What is the K p ( for the reaction? N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g )<\/a><\/p>\n

The equilibrium constant for the reaction N 2 ( g ) + O 2 ( g ) \u21cc 2 NO ( g ) at temperature (T) is 4 \u00d7 10 – 4 The value of K. for the reaction NO ( g ) \u21cc 1 2 N 2 ( g ) + 1 2 O 2 ( g ) at the same temperature is<\/a><\/p>\n

The equilibrium constant K p for the following reaction at 191 o C is 1.24. what is K c .? B ( s ) + 3 2 F 2 ( g ) \u21cc BF 3 ( g )<\/a><\/p>\n

For the equilibrium SO 2 Cl 2 ( g ) \u21cc SO 2 ( g ) + Cl 2 ( g ) what is the temperature at which K p ( atm ) K c ( M ) = 3 ?<\/a><\/p>\n

For tie reversible reaction, N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) at 500 o C the value of K p is 1 . 44 \u00d7 10 – 5 when partial pressure is measured in atmospheres. The corresponding value of K c with concentration in mole litre -1 , is :<\/a><\/p>\n

The equilibrium constant for the reaction N 2 ( g ) + O 2 ( g ) \u21cc 2 NO ( g ) is 4 \u00d7 10 – 4 at 2OOK. In presence of a catalyst, equilibrium is attained ten times faster. Therefore, the equilibrium constant in presence of the catalyst at 200 K is :<\/a><\/p>\n

For the reaction H 2 ( g ) + I 2 ( g ) \u21cc 2 HI ( g ) the equilibrium constant changes with :<\/a><\/p>\n

Consider the reactions (i) 2 CO ( g ) + 2 H 2 O ( g ) \u21cc 2 CO 2 ( g ) + 2 H 2 ( g ) ; Eqm. Constant = K 1 (ii) CH 4 ( g ) + H 2 O ( g ) \u21cc CO ( g ) + 3 H 2 ( g ) ; Eqm. Constant = K 2 (iii) CH 4 ( g ) + 2 H 2 O ( g ) \u21cc CO 2 ( g ) + 4 H 2 ( g ) ; Eqm. Constant = K 3 Which of the following relation is correct?<\/a><\/p>\n

The equilibrium constant (K. c ) for the reaction 2 HCl ( g ) \u21cc H 2 ( g ) + Cl 2 ( g ) is 4 \u00d7 10 – 34 at 25 \u00b0 C . What is the equilibrium constant for the reaction? 1 2 H 2 ( g ) + 1 2 Cl 2 ( g ) \u21cc HCl ( g )<\/a><\/p>\n

In the reaction X ( g ) + Y ( g ) \u21cc 2 Z ( g ) 2 mole of X, 1 mole of y and 1 mole of Z are placed in a 10 liter vessel and allowed to reach equilibrium. If final concentration of Z is 0.2 M, then K c for the given reaction is :<\/a><\/p>\n

9.2 grams of N 2 O 4 ( g ) is taken in a closed one liter vessel and heated till the following equilibrium is reached N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) At equilibrium, 50 % N 2 O 4 ( g ) is dissociated. What is the equilibrium constant (in mol litre -1 ) (molecular weight of N 2 O 4 = 92<\/a><\/p>\n

Two moles of NH 3 when put into a previously evacuated vessel (one liter), partially dissociated into N 2 and H 2. If at equilibrium one mole of NH 3 , is Present, the equilibrium constant is :<\/a><\/p>\n

In the presence of excess of anhydrous SrCl 2 , the amount of water taken Up is governed by K p = 10 12 atm – 4 for the following reaction at 273 K SrCl 2 \u00b7 2 H 2 O ( s ) + 4 H 2 O ( g ) \u21cc SrCl 2 \u00b7 6 H 2 O ( s ) what is equilibrium vapour pressure (in torr) of water in a closed vessel that contains SrCl 2 \u00b7 2 H 2 O ( s ) ?<\/a><\/p>\n

CuSO 4 \u00b7 5 H 2 O ( s ) \u21cc CuSO 4 \u00b7 3 H 2 O ( s ) + 2 H 2 O ( g ) ; K p = 4 \u00d7 10 – 4 atm 2 If the vapour pressure of water is 38 torr then percentage of relative humidity is : (Assume all data at constant temperature)<\/a><\/p>\n

NH 4 HS ( s ) \u21cc NH 3 ( g ) + H 2 S ( g ) the equilibrium Pressure at 25 o C is 0.660 atm. what is K p for the reaction?<\/a><\/p>\n

At 87 \u2218 C the following equilibrium is established. H 2 ( g ) + S ( s ) \u21cc H 2 S ( g ) ; K c = 0 .08 If 0.3 mole hydrogen and 2 mole sulphur are heated to 87 o C in a 2 L vessel, what will be the concentration of H 2 S at equilibrium?<\/a><\/p>\n

A + B \u21cc C + D If initially the concentration of A and B are both equal but at equilibrium concentration of D will be twice of that of A then what will be the equilibrium constant of reaction ?<\/a><\/p>\n

The equilibrium constant K c for the reaction SO 2 ( g ) + NO 2 ( g ) \u21cc SO 3 ( g ) + NO ( g ) is 16 . If 1 mole of each of all the four gases is taken in 1dm 3 vessel, the equilibrium concentration of NO would be :<\/a><\/p>\n

A catalyst increases the rate of a reaction by :<\/a><\/p>\n

At 273 K and 1atm, 10 liter of N 2 O 4 decomposes to NO 2 , according to equation N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) what is degree of dissociation (alpha) when the original volume is 25% less than that of existing volume?<\/a><\/p>\n

At certain temperature compound.AB 2 (g) dissociates according to the reaction 2 AB 2 ( g ) \u21cc 2 AB ( g ) + B 2 ( g ) With degree of dissociation \u03b1 , which is small compared with unity. The expression of K p in terms of \u03b1 and initial pressure P is :<\/a><\/p>\n

The equilibrium constant k p for the reaction H 2 ( g ) + CO 2 ( g ) \u21cc H 2 O ( g ) + CO ( g ) is 4.0 at 1660 o c. Initially 0.80 mole H 2 , and 0.80 mole CO 2 , are injected into a 5.0 liter flask. What is the equilibrium concentration of CO 2 ( g ) ?<\/a><\/p>\n

A nitrogen-hydrogen mixture initially in the molar ratio of 1 : 3 reached equilibrium to form ammonia when 25% of the N, and H, had reacted. If the total pressure of the system was 21atm, the partial pressure of ammonia at the equilibrium was<\/a><\/p>\n

Ammonia under a pressure of 15atm at 27 o C is heated to 347 o C in a closed vessel in the presence of a catalyst. Under the conditions, NH 3 is partially decomposed according to the equation, 2 NH 3 \u21cc N 2 + 3 H 2 the vessel is such that the volume remains effectively constant where as pressure increases to 50 atm. Calculate the percentage of NH 3 . actually decomposed :<\/a><\/p>\n

N 2 ( g ) + 3 H 2 ( g ) \u21cc 2 NH 3 ( g ) For the reaction initially the mole ratio was 1 : 3 of N 2 , : H 2 . At equilibrium 50% of each has reacted. If the equilibrium pressure is -Q the partial pressure of NH 3 , at equilibrium is<\/a><\/p>\n

For the reaction H 2 ( g ) + CO 2 ( g ) \u21cc CO ( g ) + H 2 O ( g ) If the initial concenffation of H 2 = CO 2 = 1 M and x moles,\/litre of hydrogen is consumed at equilibrium, the correct expression of K p is<\/a><\/p>\n

2.0 mole of PCl 5 were introduced in a vessel of 5.0 L capacity of a particular temperature. At equilibrium, PCl 5 was found to be 35% dissociated into PCl 3 and Cl 2 The value of K c for the reaction PCl 3 ( g ) + Cl 2 ( g ) \u21cc PCl 5 ( g )<\/a><\/p>\n

At 27 o and 1atm pressure, N 2 O 4 is 20 % dissociation into NO 2 What is the density of equilibrium mixture of N 2 O 4 and NO 2 at 27 \u2218 C at 27 o ‘C and 1atm?<\/a><\/p>\n

COCI 2 gas dissociates according to the equation, COCl 2 ( g ) \u21cc CO ( g ) + Cl 2 ( g ) when heated to 700 K the density of the gas mixture at 1.16atm and at equilibrium is 1.16 g\/liter. The degree of dissociation of COCl 2 at 700 K is.<\/a><\/p>\n

The degree of dissociation of l 2 molecule of 1000 o C and under atmospheric pressure is 40% by volume. If the dissociation is reduced to 20% at the same temp. total equilibrium pressure on the gas is :<\/a><\/p>\n

Determine the value of equilibrium constant (K c ) for the reaction A 2 ( g ) + B 2 ( g ) \u21cc 2 AB ( g ) If 10 moles of A; 15 moles of B, and 5 moles of, AB are placed in a 2 liter vessel and allowed to come to equilibrium. The final concentration of AB is 7.5 M<\/a><\/p>\n

At 87 \u2218 C following equilibrium is established H 2 ( g ) + S ( s ) \u21cc H 2 S ( g ) ; K p = 7 \u00d7 10 \u2212 2 If 0.50 mole of hydrogen and 1.0 mole of sulphur are heated to 87 o C in 1.0 L vessel, what will be the partial pressure of H 2 S at equilibrium?<\/a><\/p>\n

For the reaction SnO 2 ( s ) + 2 H 2 ( g ) \u21cc 2 H 2 O ( g ) + Sn ( l ) calculate K p at at 900 K where the equilibrium steam-hydrogen mixture was 45% H 2 by volume<\/a><\/p>\n

Fe 2 O 3 ( s ) may be converted to Fe by the reaction Fe 2 O 3 ( s ) + 3 H 2 ( g ) \u21cc 2 Fe ( s ) + 3 H 2 O ( g ) for which K c = 8 at temp. 720 o C What percentage of the H 2 remains unreacted after the reaction has come to equilibrium?<\/a><\/p>\n

AB 3 (g) is dissociates as AB 3 ( g ) \u21cc AB 2 ( g ) + 1 2 B 2 ( g ) ,when the initial pressure of ,AB 2 , is 800 torr and the total pressure developed at equilibrium is 900 torr. ‘what fraction of AB 3 (g) is dissociated?<\/a><\/p>\n

At 1000 K, a sample of pure NO, gas decomposes as : 2 NO 2 ( g ) \u21cc 2 NO ( g ) + O 2 ( g ) The equilibrium constant K p is 156.25 atm. Analysis shows that the partial pressure of O 2 is 0.25atm at equilibrium. The partial pressure of NO 2 , at equilibrium is :<\/a><\/p>\n

Pure nitrosyl chloride (NOCI) gas was heated to 240 o C in a 1.0 L container. At equilibrium the total pressure was 1.0atm and the NOCI pressure was 0.64 atm. What would be the value of K p ?<\/a><\/p>\n

For the dissociation reaction N 2 O 4 ( g ) \u21cc 2 NO 2 ( g ) , the degree of dissociation ( \u03b1 ) in terms of K p and total equilibrium pressure P is :<\/a><\/p>\n

For the reaction (I) and (II) ( I ) A ( g ) \u21cc B ( g ) + C ( g ) ; ( II ) X ( g ) \u21cc 2 Y ( g ) Given, K P I : K P II = 9 : 1 If the degree of dissociation of A(g) and X(g) be same then the total pressure at equilibrium (I) and (II) are in the ratio :<\/a><\/p>\n

Consider the following reactions. In which cases is product formation favoured by decreased temperature? (1) N 2 ( g ) + O 2 ( g ) \u21cc 2 NO ( g ) ; \u0394H \u2218 = 181 kJ (2) 2 CO 2 ( g ) \u21cc 2 CO ( g ) + O 2 ( g ) ; \u0394H \u2218 = 566 kJ (3) H 2 ( g ) + Cl 2 ( g ) \u21cc 2 HCl ( g ) ; \u0394H \u2218 = \u2212 9 .4 kJ (4) H 2 ( g ) + F 2 ( g ) \u21cc 2 HF ( g ) ; \u0394H \u2218 = \u2212 541 kJ<\/a><\/p>\n

The conversion of ozone into oxygen is exothermic. Under what conditions is ozone the most stable? 2 O 3 ( g ) \u21cc 3 O 2 ( g )<\/a><\/p>\n

A schematic plot of ln K eq versus inverse of temperature for a reaction is shown below the reaction must be :<\/a><\/p>\n

The most stable oxides of nitrogen will be :<\/a><\/p>\n

For the equilibrium CO (g) + 3 H 2(g) \u21cc CH 4(g) + H 2 O (g) , K c = 0.176 at 1500 0 C. The value of K p at 1500 0 C is<\/a><\/p>\n","protected":false},"excerpt":{"rendered":"

Which one of the following statements is incorrect about chemical equilibrium? For the reversible reaction, A \u21cc \u2009 2 B […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_yoast_wpseo_focuskw":"Chemical Equilibrium","_yoast_wpseo_title":"Important Chemical Equilibrium Questions for CBSE Class 11th | Chemistry","_yoast_wpseo_metadesc":"Get Important Chemical Equilibrium Questions for CBSE Class 11th here for free. 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