Refer to CBSE Class 11 Chemistry Chemical Equilibrium MCQs Set B provided below available for download in Pdf. The MCQ Questions for Class 11 Chemistry with answers are aligned as per the latest syllabus and exam pattern suggested by CBSE, NCERT and KVS. Chapter 7 Equilibrium Class 11 MCQ are an important part of exams for Class 11 Chemistry and if practiced properly can help you to improve your understanding and get higher marks. Refer to more Chapter-wise MCQs for CBSE Class 11 Chemistry and also download more latest study material for all subjects
MCQ for Class 11 Chemistry Chapter 7 Equilibrium
Class 11 Chemistry students should refer to the following multiple-choice questions with answers for Chapter 7 Equilibrium in Class 11.
Chapter 7 Equilibrium MCQ Questions Class 11 Chemistry with Answers
Question: Consider the exothermic reaction: [Consider initially only CoCl2−4 (aq) will increase]
a. If HCl is added to above equilibrium then concentration of CoCl2−4 (aq) will increase
b. On dilution with water, the concentration of CoCl2−4 (aq) will decrease
c. On doubling the volume of solution by addition of water the final concentration of [Co (H2 O) 6]2+ will be more than before equilibrium concentration
d. On increasing temperature the concentration of CoCl2−4 (aq) will decrease
Answer : A, B
Question: For the gas phase reaction carried out in vessel, the equilibrium concentration of C2H4 can be increased by:
a. Increasing the temperature
b. Decreasing the pressure
c. Adding some H2
d. Adding some C2 H6
Answer : A, B, D
Question: For the reaction 2SO3 ⇌ 2SO2 + O2 The forward reaction at constant temperature is favoured by:
a. Introducing an inert gas at constant volume
b. Introducing SO2 gas at constant volume
c. Increasing the volume of the container
d. Introducing SO3 at constant volume
Answer : C, D
Question: For the given reversible endothermic reactions taking place in a closed vessel
Reaction I Reaction II Reaction II
A ⇌ B A ⇌ C B ⇌ C
Equilibrium constants are K1 , K2 , K3 respectively:
a. ΔH is higher for the reaction III
b. Concentration of B increases with increase in temperature at constant volume
c. Mole fraction of A at equilibrium is 1 / 1 + K1 + K2
d. With increase in temperature the ratio [B]/[C] decreases
Answer : C, D
Question: When NaNO3 is heated in a closed vessel, O2 is liberated and NaNO2 is left behind. At equilibrium?
a. Addition of NaNO3 favours forward reaction
b. Addition of NaNO2 favours reverse reaction
c. Increasing pressure favours reverse reaction
d. Increasing temperature favours forward reaction
Answer : ALL
Question: The formation of NO2 in the reaction 2NO + O2 ⇌ 2NO2 + heat is favoured by:
a. Low pressure
b. High pressure
c. Low temperature
d. Reduction in the mass of
Answer : B, C
Question: Two gaseous equilibria SO2(g) + (1/2) O2(g) ⇌ SO3(g) and 2SO3(g) ⇌ 2SO2(g) +O2(g) have equilibrium constants K1 and K2 respectively at 298K.Which of the following relationships between K1 and K2is correct?
a. K1 = K2
b. K2 = K21
c. K2 = 1/K21
d. K2 = 1/K1
Answer : C
Question: For the reaction: A + B + Q ⇌ C+ D, if the temperature is increased, then concentration of the products will:
a. Increase
b. Decrease
c. Remain same
d. Become Zero
Answer : A
Question: H2(g) I2(g) ∂ ⇌ 2HI(g) In this reaction when pressure increases, the reaction direction:
a. Does not change
b. Forward
c. Backward
d. Decrease
Answer : A
Question: The rate of reaction of which of the following is not affected by pressure?
a. PCl3 + Cl2 ⇌ PCl5
b. N2 + 3H2 ⇌ 2NH3
c. N2 + O2 ⇌ 2NO
d. 2 2 3 2SO +O ⇌ 2SO3
Answer : C
Question: The formation of nitric oxide by contact process N2 + O2 ⇌ 2NO. Δ H = 43.200 kcal is favoured by:
a. Low temperature and low pressure
b. Low temperature and high pressure
c. High temperature and high pressure
d. High temperature and excess reactants concentration
Answer : D
Question: Which reaction is not effected by change in pressure?
a. H2 + I2 ⇌ 2HI
b. 2C + O2 ⇌ 2CO
c. N2 + 3H2 ⇌ 2NH3
d. PCl5 ⇌ PCl3 + CI2
Answer : A
Assertion and Reason
Note: Read the Assertion (A) and Reason (R) carefully to mark the correct option out of the options given below:
a. If both assertion and reason are true and the reason is the correct explanation of the assertion.
b. If both assertion and reason are true but reason is not the correct explanation of the assertion.
c. If assertion is true but reason is false.
d. If the assertion and reason both are false.
e. If assertion is false but reason is true.
Question: Assertion: Kp = Kc for all reaction.
Reason: At constant temperature, the pressure of the gas is proportional to its concentration.
Answer : E
Question: Assertion: On cooling a freezing mixture, colour of the mixture turns to pink from deep blue for a reaction. Co(H2 O)2+6 (aq) + 4Cl−(aq) ⇌ CoCl2-4(aq) − + 6H2 O(l) .
Reason: Reaction is endothermic so on cooling, the reaction moves to backward direction.
Answer : A
Question: Assertion: If Qc (reaction quotient) < KC (equilibrium constant) reaction moves in direction of reactants.
Reason: Reaction quotient is defined in the same way as equilibrium constant at any stage of the reaction.
Answer : E
Question: Assertion: NaCl solution can be purified by passage of hydrogen chloride through brine.
Reason: This type of purification is based on Lehaterlier's principle.
Answer : C
Question: Assertion: Equilibrium constant has meaning only when the corresponding balanced chemical equation is given.
Reason: Its value changes for the new equation obtained by multiplying or dividing the original equation by a number.
Answer : A
Question: Assertion: Catalyst affects the final state of the equilibrium.
Reason: It enables the system to attain a new equilibrium state by complexing with the reagents.
Answer : D
Question: Assertion: For the reaction, 2NH3 (g) ⇌ N2 (g) +3H2 (g), the unit of Kp will be atm.
Reason: Unit of Kp is (atm)Δn.
Answer : E
Question: Assertion: Effect of temperature of Kc or Kp depends on enthalpy change.
Reason: Increase in temperature shifts the equilibrium in exothermic direction and decrease in temperature shifts the equilibrium position in endothermic direction.
Answer : C
Question: Assertion: For a gaseous reaction, xA + yB ⇌ lC + mD, Kp = KC.
Reason: Concentration of gaseous reactant is taken to be unity.
Answer : D
Question: Assertion: SO2 (g) + 1/2 O2 (g) ⇌ SO3 (g) + heat. Forward reaction is favoured at high temperature and low pressure.
Reason: Reaction is exothermic.
Answer : E
Comprehension Based
Paragraph-I
Decomposition of ammonium chloride is an endothermic reaction. The equilibrium may be represented as: NH4 Cl(s) ⇌ NH3 (g) + HCl(g) A 6.250 g sample of NH4 Cl is placed in an evaculated 4.0. L container at 27°C. After equilibrium the total pressure inside the container is 0.820 bar and some solid remains in the container. Answer the followings.
Question: The value of Kp for the reaction at 300 K is:
a. 16.2
b. 0.168
c. 1.68
d. 32.4
Answer : B
Question: The amount of solid NH4 Cl left behind in the container at equilibrium is:
a. 2.856
b. 28.56
c. 0.2856
d. 1.320
Answer : A
Question: If the volume of container were doubled at constant temperature, then what would happen to the amount of solid in the container?
a. Decrease
b. Increases
c. Remain unchanged
d. None
Answer : A
Question: The extent of decomposition can be increased by:
a. Increasing the temperature
b. Decreasing the temperature
c. Adding more NH4 Cl
d. Removing HCl(g)
Answer : A
Question: The value of Kp for the reaction decreases with:
a. Increase in volume
b. Decrease in temperature
c. Decrease in pressure
d. Increase in temperature
Answer : B
Integer
Question: When PCl5 is heated it dissociates into PCl3 and Cl2. The density of the gas mixture at 200ºC and at 250ºC is 70.2 and 57.9 respectively. Find the degree of dissociation at 200ºC and 250ºC:
Answer : 1
Question: The degree of dissociation of PCl5 is 60%, then find out the observed molar mass of the mixture:
Answer : 129
Question: At 444ºC 15g mole of hydrogen are mixed with 5.2g mole of I2 vapour. When equilibrium was established,10g mole of HI was formed. Calculate the equilibrium constant for the reaction?
Answer : 50
Question: The degree of dissociation is 0.4 at 400K and 1 atm for the gaseous reaction PCl5 ⇌ PCl3 + Cl2 Assuming ideal behaviour of all the gases, calculate the density of equilibrium mixture at 400K and 1 atm pressure: (Atomic mass of P =31 and Cl =35.5)
Answer : 5
Question: The value of Kp for the reaction 2H2 O(g) + 2Cl2 (g) ⇌ 4HCl(g) + O2 (g) is 0.035 atm at 400°C, when the partial pressures are expressed in atmosphere. Calculate c K for the reaction, (1/2) O2 (g) 2HCl(g) ⇌ Cl2 (g) + H2 O(g) ?
Answer : 40
Match the Column
Question: The section questions each with two columns I and II.
Match the items given in column I with that of column II.
Column I Column II
(A) Q = K 1. Reaction is nearer to com-pletion
(B) Q < K Q < K 2. Reaction is not at equilibrium
(C) Q > K 3. Reaction is fast in forward direction
(D) K >>> l 4. Reaction at equilibrium
5. Reaction proceeds in back-ward direction
a. A→4; B→2-3; C→2-5; D→1
b. A→2; B→4; C→3; D→1
c. A→1; B→3; C→2; D→4
d. A→4; B→1; C→3; D→2
Answer : A
Question: Match the statement of Column I with those in Column II:
Column I Column II
(A) CaCO3 (s) ⇌ CaO(s) + CO2 (g) 1. moL−1
(B) NH4 Cl(g) ⇌ NH3 (g) + HCl(g) 2. Unitless
(C) H2 (g) + I2 (g) ⇌ 2HI(g) 3. atm
(D) N2 (g) + 3H2 (g) ⇌ 2NH3 (g) 4. atm−2
a. A→1-3; B→1-3; C→2; D→4
b. A→2; B→4; C→3; D→1
c. A→1; B→3; C→2; D→4
d. A→4; B→1; C→3; D→2
Answer : A
Question: Match the statement of Column I with those in Column II:
Column I Column II
(A) Reaction is reversed . 1. (K)1 / 2
(B) Reaction is divided by 2 2. K2
(C) Reaction is multiplied by 2 3. 1 / K
a. A→3; B→1; C→2
b. A→2; B→4; C→3
c. A→1; B→3; C→2
d. A→3; B→1; C→3
Answer : A
I. MCQ - Choose Appropriate Alternative
1. At equilibrium the rate of forward reaction and the rate of reverse reaction are __________. (Equal, Changing, Different)
2. Such reactions, which proceed to forward direction only and are completed after sometime are called __________ reaction. (Irreversible, Reversible, Molecular)
3. Such reactions, which proceed to both the direction and are never completed, are called __________ reaction. (Irreversible, Reversible, Molecular)
4. The rate of chemical reaction is directly proportional to the product of the molar concentration of __________. (Reactants, Products, Both reactants and products)
5. “If a system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of this stress. This principle is known as __________. (Le-Chatelier’s Principle, Gay Lussac’s Principle, Avogadro’s Principle)
6. A very large value of Kc indicates that reactants are __________. (very stable, unstable, moderately stable)
7. A very low value of Kc indicates that reactants are __________. (very stable, very unstable, moderately stable)
8. The equilibrium in which reactants are products are in single phase is called __________. (Homogenous Equilibrium, Heterogenous Equilibrium, Dynamic Equilibrium)
9. The equilibrium in which reactants and products are in more than one phases are called __________. (Homogenious Equilibrium, Heterogenious Equilibrium, Dynamic Equilibrium)
10. Chemical Equilibrium is __________ equilibrium. (Dunamic, Static, Heterogeneous)
11. In exothermic reaction, lowering of temperature will shift the equilibrium to __________. (right, left, equally on both the direction)
12. In endothermic reaction, lowering of temperature will shift the equilibrium to __________. (right, left, equally on both the direction)
13. A catalyst __________ the energy of activation. (increases, decreases, has no effect on)
14. At equilibrium point __________. (forward reaction is increased, backward reaction is increased, forward and backward reactions become equal)
15. NH3 is prepared by the reaction N2 + 3H2 → 2NH3 ; ΔH = -21.9 Kcal. The maximum yield of NH3 is obtained __________. (At low temperature and high pressure, at high temperature and low pressure, at high temperature and high pressure)
16. When a high pressure is applied to the following reversible process: N2 + O2 →2NO The equilibrium will __________ (shift to the forward direction, shift to the backward direction, not change)
17. The value of Kc __________ upon the initial concentration of the reaction. (depends, partially depends, does not depend)
18. While writing the Kc expression, the concentration of __________ are taken in the numerator.
19. Solubility product constant is denoted by __________. (Kc, Ksp, Kr)
20. “The degree of ionization of an electrolyte is suppressed by the addition of another electrolyte containing a common ion.” This phenomenon is called __________. (Solubility Product, Common Ion Effect, Le-Chatelier’s Principle)
II. Fill in the Blanks
1. The reactions, which proceed in both the directions, are called __________ reactions.
2. The reactions, which proceed to one direction only, are called __________ reactions.
3. Reversible reactions are __________ completed.
4. Irreversible reactions are __________ after some time.
5. A reversible reaction is said to be in __________ when the rate of forward reaction becomes equal to the rate of backward reaction.
6. The concentrations of reactants and products are __________ at equilibrium point.
7. The value of Kc depends upon the __________ of the reactants.
8. A increase of the value of Kc tends to move the reaction to the __________ direction.
9. A decrease of the value of Kc tends to move the reaction to the __________ direction.
10. An increase in the concentration of the reactants will move the reaction to the __________ direction.
11. A decrease in the concentration of the reactants will move the reaction to the __________ direction.
12. Equilibrium constant is denoted by __________.
13. When the equilibrium constant value is very __________, we can conclude that the forward reaction is almost completed.
14. When equilibrium constant value is very __________ we can conclude that forward reaction will occur to very little extent.
15. According to __________ principle, if system in equilibrium is subjected to a stress, the equilibrium shifts in a direction to minimize or undo the effect of the stress.
16. In exothermic reaction, the __________ of temperature favour the forward rate of reaction.
17. In endothermic reactions, the __________ of temperature favour the forward rate of reaction.
18. A __________ is a substance which effects the rate of reaction but remains unaltered at the end of the reaction.
19. A catalyst increases the velocity of the reaction by decreasing the __________.
20. The suppression of degree of ionization of a sparingly soluble weak electrolyte by the addition of a strong electrolyte containing an ion in common is called __________.
21. __________ is purified in industries by Common Ion Effect.
22. A reaction moves to the left when the concentrations of the products are __________.
23. A reaction moves to the right when the concentrations of the products are __________.
24. Increase in pressure will move the reaction in the direction of __________ volume.
25. Decrease in pressure will move the reaction in the direction of __________ volume.
26. An increase of temperature favours the formation of products in case of __________ reaction.
27. A decrease of temperature fovours the formation of products in case of __________ reaction.
28. Heating moves an endothermic reaction to the __________.
29. Cooling move an exothermic reaction to the __________.
30. The product of ionic concentration in a saturated solution is called __________ constant.
31. When HCl is added to NaCl, the concentration of __________ ion is increased.
32. Chemical reaction involving the substances in more than one phases are called __________.
33. The formation of NH3 is exothermic process hence __________ temperature will favour the formation of NH3.
34. The formation of NO from N2 and O2 is endothermic process hence __________ temperature will favour the formation of NO.
35. Chemical Equilibrium is __________ equilibrium.
36. Molar concentration is also called __________.
37. The rate at which a substance takes part in a chemical reaction depends upon its __________.
38. __________ principle is applied to all reversible reaction.
39. A common ion __________ the solubility of the salt.
40. Number of moles present per dm3 of a substance is called __________.
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MCQs for Chapter 7 Equilibrium Chemistry Class 11
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