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AP Chemistry 5.3: Integrated Rate Laws

Practice AP Chemistry questions on identifying reaction order from concentration-time graphs, applying integrated rate laws, calculating k, and interpreting first-order half-life.

Syllabus
Effective Fall 2025
Course
AP Chemistry

Exam points

  • Explain how reaction rates depend on collisions, activation energy and reaction pathways.
  • Apply rate laws and concentration data to determine reaction order and predict concentration changes.

5.3.A—Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction… 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.A—Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction… question 1 — AP Chemistry
Figure for Question 5.3.A—Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction… 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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