CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs
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CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs (SET A)
1. In lime kiln, reversible reaction CaCO3(s) ⇄ CaO(s) + CO2(g) proceeds to completion because
(A) High temperature
(B) CO2 escapes
(C) CaO removed
(D) Low temperature
Answer: CO2 escapes.
2. In thermal decomposition of potassium chlorate gives as 2KClO3 → 2KCl + 3O2. Law of mass action
(A) Cannot be applied
(B) Can be applied
(C) Can be applied at low temperature
(D) None
Answer: Cannot be applied.
3.What is active mass of 64 g of HI in a 2 L flask? (At. wt. of I = 127)
(A) 1
(B) 2
(C) 5
(D) 0.25
Answer: 0.25.
4. Chemical equilibrium is dynamic in nature because
(A) Both forward and backward reactions occur at all times with same speed
(B) Equilibrium is maintained rapidly
(C) Maintained slowly
(D) none
Answer: Both forward and backward reactions occur at all times with same speed.
5. Select the chemical reaction which is irreversible?
(A) H2 + I2 ⇄ 2HI
(B) O2 + 2SO2 ⇄ 2SO3
(C) CaCO3 ⇄ CaO + CO2
(D) AgNO3 + NaCl ⇄ NaNO3 + AgCl
Answer: AgNO3 + NaCl ⇄ NaNO3 + AgCl.
CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs (SET B)
1. Which of the following statements regarding a chemical equilibrium is wrong?
(A) An equilibrium can be shifted by altering temperature or pressure
(B) An equilibrium is dynamic
(C) Forward reaction is favoured when catalyst is added
(D) Same state of equilibrium is reached, whether one starts from reactants or products
Answer: Forward reaction is favoured when catalyst is added.
2. A reversible reaction having two reactants in equilibrium if the concentration of reactants are doubled, the equilibrium constant will
(A) Become 4 times
(B) Become ¼ th times
(C) Become 1/16 th times
(D) Remains the same
Answer: Remains the same.
3. For the hypothetical reactions, the equilibrium constant (K) values are given
A ⇄ B, K1
B ⇄ C,K2
C ⇄ D, K3
The equilibrium constant (K) for the reaction A ⇄ D is
(A) K1 + K2 + K3
(B) K1. K2. K3
(C) K1 + K2 – K3
(D)None
Answer: K1. K2. K3.
4. The unit of Kp in the following reaction is
N2(g) + 3H2(g) ⇄ 2NH3(g)
(A) atm
(B) atm–2
(C) atm2
(D) atm–1
Answer: atm–2.
5. Reaction A(g) + B(g) ⇄ C(g) + D(g). If the concentration of A is doubled then
(A) Equilibrium constant (Kc) will be doubled
(B) Equilibrium constant (Kc) will be halved
(C) Equilibrium constant (Kc) remains unaffected
(D) Equilibrium constant (Kc) will become four times
Answer: Equilibrium constant (Kc) remains unaffected.
CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs (SET C)
1. For the reaction A + B ⇄ 2C, at the equilibrium concentration of A and B each is 0.20 mole/liter and concentration C is observed as 0.60 mol/liter. Equilibrium constant (Kc)
(A) 9
(B) 18
(C) 6
(D) 24
Answer: 9.
2. The endothermic reaction M + N ⇄ P is allowed to attain an equilibrium at 25°C. Formation of P can be increased by
(A) Raising temperature
(B) Lowering temperature
(C) Keeping temperature constant
(D) Decreasing the conc. of M and N
Answer: Raising temperature.
3. Formation of nitric oxide by contact process N2 + O2 ⇄ 2NO.ΔH = 43.2 Kcal is favoured by
(A) Low T and low P
(B) Low T and high P
(C) High T and high P
(D) High T and excess reactants conc.
Answer: High T and excess reactants conc.
4. In which of the following does the reaction go almost to completion?
(A) A + B ⇄ C; K = 10^4
(B) X + Y ⇄ Z; K = 10^–3
(C) P + Q ⇄ R; K = 1
(D) M + N ⇄ O + P; K = 10^–1
Answer: A + B ⇄ C; K = 10^4.
5. At constant pressure, the addition of argon in Haber’s process
(A) Reduces the formation of ammonia from N2 and H2
(B) Increase the formation of ammonia from N2 and H2
(C) None
(D) Reduces the dissociation of ammonia
Answer: Reduces the formation of ammonia from N2 and H2.
CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs (SET D)
1. Pure NH3 is placed in a vessel at a temperature where its dissociation is appreciable. At equilibrium
(A) Kp does not change significantly with pressure
(B) Concentration of N2 does not change with pressure
(C) Concentration of NH3 does not change with pressure
(D) none
Answer: Kp does not change significantly with pressure.
2. For the equilibrium CO2 + H2O ⇄ CO2 + H2 The relation between Kp and Kc at 25°C and at 100°C are
(A) Kp = Kc, Kp = Kc
(B) Kp = Kc(RT)–1, Kp = Kc
(C) Kp = Kc(RT), Kp = Kc(RT)
(D) Kp = Kc(RT), Kp = Kc
Answer: Kp = Kc(RT), Kp = Kc.
3. The oxidation of SO2 by O2 to SO3 is an exothermic reaction. The yield of SO3 will be maximum if
(A) Temperature is increased and pressure is kept constant
(B) Temperature is reduced and pressure is increased
(C) Both temperature and pressure are increased
(D) Both temperature and pressure are reduced
Answer: Temperature is reduced and pressure is increased.
4. For the given equilibrium reaction CaCO3(s) ⇄ CaO(s) + CO2(g). The addition of more CaCO3(s) causes
(A) The decrease in the concentration of CO2(g)
(B) The increase in the concentration of CO2(g)
(C) No change in the concentration of CO2(g)
(D) Increase in the concentration of CaO(s)
Answer: No change in the concentration of CO2(g).
5. Identify the reaction which is not affected by increase in pressure.
(A) N2(g) + O2 ⇄ 2NO(g)
(B) 2SO2(g) + O2(g) ⇄ 2SO3(g)
(C) PCl5(g) ⇄ PCl3(g) + Cl2(g)
(D) N2(g) + 3H2(g) ⇄ 2NH3(g)
Answer: N2(g) + O2 ⇄ 2NO(g).
CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs (SET E)
1. The equilibrium 2SO2(g) + O2(g) ⇄ 2SO3(g), shift in forward direction if
(A) Catalyst is added
(B) Large amount of product is used.
(C) Small amounts of reactants are used
(D) none
Answer: none.
1. When NaNO3(s) is heated in closed vessel, oxygen is liberated and NaNO2(s) is left behind. At equilibrium
(A) Addition of NaNO2(s) favours reverse reaction
(B) Addition of NaNO3(s) favours forward reaction
(C) Decreasing temperature favours forward reaction
(D) Increasing pressure favours reverse reaction
Answer: Increasing pressure favours reverse reaction.
2. Which of the following reactions will be favoured by high pressure?
(A) H2(g) + l2(g) ⇄ 2Hl(g)
(B) PCl5(g) ⇄ PCl3(g) + Cl2(g)
(C) N2(g) + 3H2(g) ⇄ 2NH3(g)
(D) N2(g) + O2(g) ⇄ 2NO(g)
Answer: N2(g) + 3H2(g) ⇄ 2NH3(g).
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