AP Chemistry Kinetics Practice

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Answer the following questions. You may use your periodic table and reference sheet, but calculator use is not permitted.

The rate law for the reaction represented by the equation below is rate = k[H₂][ICl]. Which of the following could be the first elementary step of a two step mechanism if the first step is slow and the second step is fast? *

1 point

Option 1

Option 2

Option 3

Option 4

2A + B ⟶ A₂B Consider the reaction represented above. During an experiment in which a large excess of reactant B was present, the concentration of reactant A was monitored over time. A plot of 1/[A] versus time is shown in the figure below. What is the order of reaction with respect to reactant A? *

1 point

zero order

first order

second order

third order

Which of the following will most likely increase the rate of the reaction represented below? Cl₂(g) + 3 F₂(g) ⟶ 2 ClF₃(g) *

1 point

Adding Ar(g) to the reaction system

Removing some Cl2(g) from the reaction system

Increasing the volume of the reaction vessel using a piston

Increasing the temperature of the system

The equation below represents an elementary step in a chemical reaction. Which of the following is the correct expression for the rate law of the elementary step? *

1 point

Option 1

Option 2

Option 3

Option 4

The reaction for the destruction of ozone in the atmosphere and its experimentally determined rate law are represented below. Two different possible mechanisms have been proposed and are shown below. Based on the information provided, which of the following is true? *

1 point

Only mechanism 1 is consistent with the rate law.

Only mechanism 2 is consistent with the rate law.

Both mechanism 1 and mechanism 2 are consistent with the rate law.

Neither mechanism 1 and mechanism 2 are consistent with the rate law.

Which of the following best helps explain why a decrease in reactant concentration decreases the rate of a chemical reaction? *

1 point

At lower reactant concentrations, reactions have a higher activation energy.

At lower reactant concentrations, collisions between reactant particles are less frequent.

At lower reactant concentrations, reactions have a lower activation energy.

At lower reactant concentrations, collisions between reactant particles are less likely to have the correct orientation.

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