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AP Chemistry Unit 5.1: Reaction Rates

Practice AP Chemistry Unit 5.1 questions on interpreting reaction rates, collision behavior, and how concentration, temperature, surface area, and catalysts change observations.

Syllabus
Effective Fall 2025
Course
AP Chemistry

Exam points

  • Use stoichiometry and reaction equations to predict quantities, limiting reagents, yields, and composition.
  • Calculate mass, moles, concentration, and gas volume from balanced reactions and experimental measurements.

Covered syllabus points

5.1.A—Explain the relationship between the rate of a chemical reaction and experimental parameters

5.1 Reaction Rates question 1

[Maximum number: 1]

At elevated temperatures, NO2\mathrm{NO}_{2} undergoes decomposition in the gas phase, forming NO and O2\mathrm{O}_{2} as represented by the following equation.

2NO2→2NO+O22 \mathrm{NO}_{2} \rightarrow 2 \mathrm{NO}+\mathrm{O}_{2}

A scientist measures the change in [NO2]\left[\mathrm{NO}_{2}\right] over the first 100. s of the reaction at 546°C. The scientist uses the data collected from the experiment to generate the following two graphs.

Figure for Question 5.1 Reaction Rates question 1 — AP Chemistry
Figure for Question 5.1 Reaction Rates question 1 — AP Chemistry

Based on these data, the scientist makes the claim that the rate law for the reaction is rate =k[NO2]2=k\left[\mathrm{NO}_{2}\right]^{2}.

At a certain point in the reaction, the rate of disappearance of NO2\mathrm{NO}_{2} is determined to be 6.52×10−7M/s6.52 \times 10^{-7} M / \mathrm{s}. Determine the rate of appearance, in M / s, of O2\mathrm{O}_{2} at this same point in the reaction.

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