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Class 12 Chemistry MCQ Chapter 4 Chemical Kinetics
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Chemical Kinetics
Chapter: 4
| MCQ |
1. The rate of chemical reaction becomes double for every 10 deg rise in temperature because of:
(i) Decreases in activation energy.
(ii) Increase in activation energy.
(iii) Increase in number of activated molecules.
(iv) Increase in the number of molecular collisions.
Ans: (iii) Increase in number of activated molecules.
2. What defines the rate of a chemical reaction?
(i) Change in temperature over time.
(ii) Change in pressure of reactants.
(iii) Change in concentration of a reactant or product over time.
(iv) Change in the volume of the system.
Ans: (iii)Change in concentration of a reactant or product over time.
3. In a reaction, 2X → Y, the concentration of X decreases from 0.50 M to 0.38 M in 10 min. What is the rate of reaction in Ms-1 during this interval ?
(i) 2 × 10-4
(ii) 4 × 10-2
(ii) 2 × 10-2
(iv) 1 × 10-2
Ans: (i) 2 × 10-4
4. The units of the rate of a reaction, when concentration is expressed in mol L⁻¹ and time in seconds, are:
(i) Mol L⁻¹ s⁻¹
(ii) Atm s⁻¹
(iii) Mol L⁻¹
(iv) L mol⁻¹ s⁻¹
Ans: (i) Mol L⁻¹ s⁻¹
5. The rate constant of a reaction depends upon
(i) Initial concentration of the reactants.
(ii) Extent of the reaction.
(iii) Temperature of the reaction.
(iv) The time of completion of reaction.
Ans: (iii) Temperature of the reaction.
6. One If the concentration of a reactant decreases from 0.100 M to 0.0905 M in 50 seconds, what is the average rate of the reaction?
(i) 1.90×10−4 mol L−1s−1
(ii) 1.70×10−4 mol L−1s−1
(iii) 4.00×10−4 mol L−1s−1
(iv) 2.00×10−4 mol L−1s−1
Ans: (i) 1.90×10−4 mol L−1s−1
7. If the instantaneous rate of a reaction at t=600 s is 5.12×10−5 mol L−1s−1, what does this value represent?
(i) Average rate over 600 seconds.
(ii) Rate at which the reactant is disappearing at that moment.
(iii) Rate of formation of products over the entire reaction.
(iv) Total concentration of all species at 600 seconds.
Ans: (ii)Rate at which the reactant is disappearing at that moment.
8. In the equation Rate=k[A]x[B]y, what does the constant kkk represent?
(i) The molarity of the products.
(ii) The rate constant for the reaction.
(iii) The concentration of reactants.
(iv) The time taken for the reaction.
Ans: (ii)The rate constant for the reaction.
9. For the reaction Rate=k[CHCl3][Cl2]1/2, what is the order of the reaction with respect to CHCl3 and Cl2?
(i) The order is 1.5
(ii) The order is 2
(iii) The order is 0.5
(iv) The order is 1
Ans: (i) The order is 1.5
10. In the rate expression Rate=k[A]3/2[B]−1, what is the order of the reaction?
(i) 1
(ii) 0.5
(iii) 2
(iv) 3
Ans: (ii) 0.5
11. Which statement is true about a catalyst?
(i) It can only catalyse non-spontaneous reactions.
(ii) It alters the equilibrium constant of the reaction.
(iii) It is consumed in the reaction.
(iv) It remains unchanged after the reaction.
Ans: (iv) It remains unchanged after the reaction.
12. If a reaction between A and B to give C shows first order kinetics in A and second order in B, the rate equation can be written as:
(i) Rate = K[A] [B]
(ii) Rate K[A] [B]1/2
(iii) Rate = K[A]1/2 [B]
(iv) Rate = K[A] [B]2
Ans: (iv) Rate = K[A] [B]2
13. In a complex reaction, a sequence of elementary reactions is called:
(i) Pathway.
(ii) Mechanism.
(iii) Cycle.
(iv) Series.
Ans: (ii) Mechanism.
14. A reaction in which reactants (R) are converted into products (P) follows second order kinetics. If concentration of R is increased by four times, what will be the increase in the rate of formation of P?
(i) 6 times.
(ii) 5 times.
(iii) 16 times.
(iv) 8 times.
Ans: (iii) 16 times.
15. Reactions that take place in one step are known as:
(i) Complex reactions.
(ii) Elementary reactions.
(iii) Consecutive reactions.
(iv) Intermediate reactions.
Ans: (ii) Elementary reactions.
