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AP Chemistry Unit 5.3: Integrated Rate Laws

Practice AP Chemistry Unit 5.3 questions on interpreting concentration-time plots, applying integrated rate laws, calculating k, and using first-order half-life.

Syllabus
Effective Fall 2025
Course
AP Chemistry

Exam points

  • Use particle and equilibrium models to explain solubility, precipitation, and concentration changes in solution.
  • Calculate Ksp, ion concentrations, and reaction direction from balanced equations and measured solution data.

Covered syllabus points

5.3.A—Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction…

5.3 Concentration Changes Over Time 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 5.3 Concentration Changes Over Time question 1 — AP Chemistry
Figure for Question 5.3 Concentration Changes Over Time 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}.

Explain how the graphs indicate that the reaction is second order with respect to NO2\mathrm{NO}_{2}.

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