Le Chatelier’s Principle, Class 11 Chemistry Sample Papers

Equilibrium Page 225 Q 7.11 Class 11 CBSE Chemistry

Equilibrium Page 225 Q 7.12 Class 11 CBSE Chemistry

Equilibrium Page 225 Q 7.13 Class 11 CBSE Chemistry

Equilibrium Page 225 Q 7.14 Class 11 CBSE Chemistry

Equilibrium Page 225 Q 7.15 Class 11 CBSE Chemistry

Equilibrium Page 225 Q 7.16 Class 11 CBSE Chemistry

Equilibrium Page 226 Q 7.17 Class 11 CBSE Chemistry

Equilibrium Page 226 Q 7.18 Class 11 CBSE Chemistry

Equilibrium Page 226 Q 7.19 Class 11 CBSE Chemistry

Equilibrium Page 226 Q 7.20 Class 11 CBSE Chemistry

1. There will be total 10  MCQ in this test.
2. Please keep a pen and paper ready for rough work but keep your books away.
3. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number.
4. No negative marking for incorrect choice.
5. Please click on “Finish the Test” when you want to exit.
6. All the best – Happy Studying.

1. Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?
N₂O₄ (g) ⇔ 2NO₂ (g)

 A

 B

 C

 D

Question 1 of 10

2. For the reaction 2NO₂ (g) ⇒ N₂O₄ (g) , Kp equals

  Kc

 Kc(RT)

 Kc/RT

 RT/Kc

Question 2 of 10

3. Which one of the following is true about the reaction
CaCO₃ ⇒ CaO_(s) + CO₂H=-1050kJ

 CaO_(s) is more stable than CaCO_3(s)

 CaO_(s) is not dissociated

  It is a reversible reaction at high temperature

 The reaction takes place at low temperature

Question 3 of 10

4. The equilibrium-constant expression depends on which of the followings of the reversible reaction.

 the quantities of reactants and products initially present

 stoichiometry and mechanism

 temperature (Level-M)

 mechanism

Question 4 of 10

5. How will addition of catalyst affect the equilibrium of a reaction?

 It will sometimes shift in forward and sometimes in backward direction

 Equilibrium will shift in the backward direction

 There will be no effect on equilibrium

 Equilibrium will shift in the forward direction

Question 5 of 10

6. In a chemical equilibrium K_c = K_p when:

 The number of moles of reactant entering into the reaction is equal to the number of moles of product formed.

 The number of moles of reactant entering into the reaction is more than the number of moles of product formed

 The number of moles of reactant entering into the reaction is less than the number of moles of product formed

 The reaction is not reversible.

Question 6 of 10

7. K_c for the following reaction is 0.020 at 445°C,
2HI(g) H₂(g) + I₂(g)
A mixture of H₂, I₂, and HI in a vessel has the following equilibrium concentrations: [HI] = 2.0 M, [H₂] = 0.50 M and [I₂] = 0.10 M then which one of the following statements is true?

  Q_c is less than K_c; more HI will be produced.

 Q_c is less than K_c; more H₂ and I₂ will be produced.

 Q_c is greater than K_c; more HI will be produced.

 Q_c is greater than K_c; more H₂ and I₂ will be produced.

Question 7 of 10

8. Which one of the following is incorrect with respect to quilibrium reaction:
N₂ (g) + 3H₂ (g) —> 2NH₃ (g) , Given k_p = 1 x 10^-4

 The synthesis of ammonia is an exothermic reaction, so the rate of product formation may increase at higher temperature.

 The rate constant for the forward reaction is less than that of the reverse reaction.

 The equilibrium constant is given by KC = [NH₃]² / [N₂][H₂]³

  Conducting the reaction under high pressures will increase the yield of ammonia.

Question 8 of 10

9. The equilibrium constant for the reaction,

CaCO₃(s) CaO(s) + CO₂ (g), is

 A

 B

 C

 D

Question 9 of 10

10. When two substances(reactants) react to give products reversibly , the reaction quotient (Q) of the reaction as the reaction proceeds

  Decreases with time till equilibrium point

 Increases with time till equilibrium point

 Is independent of time

 Is zero

Question 10 of 10

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