Question 1

Which of the following best describes the focus of chemical kinetics?

Accepted Answer

The study of the rates of chemical reactions and the factors that affect them.

Question 2

A reaction is found to be first order with respect to reactant A and second order with respect to reactant B. What is the correct rate law for this reaction?

Accepted Answer

$$	ext{Rate} = k[A][B]^2$$

Question 3

In a certain reaction, doubling the concentration of reactant X causes the rate to quadruple, while doubling the concentration of reactant Y has no effect on the rate. What is the order of the reaction with respect to X and Y?

Accepted Answer

Second order with respect to X, zero order with respect to Y

Question 4

Which of the following statements about the rate constant $$k is $$correct?

Accepted Answer

The value of $$k$$ depends on temperature but not on the concentrations of reactants.

Question 5

For a first-order reaction, which of the following plots will yield a straight line?

Accepted Answer

$$\ln [A]$$ versus time

Question 6

The decomposition of a drug in the human body follows first-order kinetics. If the initial concentration is $$0.10\ \mathrm{M}$$ and the rate constant $$k is$$ $$0.20\ \mathrm{min}^{-1}$$, what is the concentration after $$10$$ minutes? (Use $$[A]_t = [A]_0 e$$^{-kt}$$)

Accepted Answer

$$0.0135\ \mathrm{M}$$

Question 7

Which of the following best explains why increasing temperature generally increases the rate of a chemical reaction?

Accepted Answer

A higher temperature increases the fraction of molecules with enough energy to overcome the activation energy barrier.

Question 8

A reaction has the following rate law: $$	ext{Rate} = k[$$BrO_3$$^-][Br^-][H^+]^2. $$What is the overall order of the reaction?

Accepted Answer

Fourth order

Question 9

Which of the following is true about a catalyst in a chemical reaction?

Accepted Answer

It provides an alternative reaction pathway with a lower activation energy.

Question 10

The Arrhenius equation is $$k = Ae$$^{-E_a/(RT)}$$. If you plot $$\ln k$$ versus 1/T$, what does the slope of the line represent?

Accepted Answer

$$-E_a/R$$

Question 11

In a multi-step reaction mechanism, which step determines the overall rate of the reaction?

Accepted Answer

The slowest (rate-determining) step

Question 12

Which of the following is a correct statement about reaction intermediates?

Accepted Answer

They are produced in one step and consumed in a later step of the reaction mechanism.

Question 13

A zero-order reaction has a rate law $$	ext{Rate} = k. If $$the initial concentration of A is $$0.50\ \mathrm{M}$$ and $$k = 0.10\ \mathrm{M\ s$$^{-1}$$}$$, how long will it take for the concentration of A to reach $$0.10\ \mathrm{M}$$?

Accepted Answer

$$4.0\ \mathrm{s}$$

Question 14

Which of the following is NOT a factor that affects the rate of a chemical reaction?

Accepted Answer

The color of the reactants

Question 15

For a second-order reaction with respect to A, what is the integrated rate law?

Accepted Answer

$$\frac{1}{[A]_t} = kt + \frac{1}{[A]_0}$$

Question 16

Which of the following best describes the role of enzymes in biological systems?

Accepted Answer

They are protein catalysts that speed up biochemical reactions by lowering the activation energy.

Question 17

A reaction is found to be zero order with respect to reactant B. What will happen to the rate if the concentration of B is doubled?

Accepted Answer

The rate will remain unchanged.

Question 18

Which of the following is a correct statement about the half-life of a first-order reaction?

Accepted Answer

It is independent of the initial concentration of the reactant.

Question 19

In the context of the collision theory, which factor does NOT affect the rate of a chemical reaction?

Accepted Answer

The color of the reactants

Question 20

A reaction has an activation energy of $$50\ \mathrm{kJ\ $$mol^{-1}$$}. If $$the temperature is increased, what will happen to the rate constant $$k$$?

Accepted Answer

It will increase.

Chemical Kinetics: Principles and Applications

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