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AP Chemistry 5.1: Reaction Rates

Practice AP Chemistry questions on explaining how concentration, temperature, surface area, and catalysts affect reaction rate, including stoichiometric links between species.

Syllabus
Effective Fall 2025
Course
AP Chemistry

Exam points

  • Explain how thermodynamic energy changes reflect bond breaking, bond forming and heat transfer in reactions.
  • Apply enthalpy, calorimetry and energy diagrams to calculate or predict heat flow in chemical processes.

5.1.A—Explain the relationship between the rate of a chemical reaction and experimental parameters 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.A—Explain the relationship between the rate of a chemical reaction and experimental parameters question 1 — AP Chemistry
Figure for Question 5.1.A—Explain the relationship between the rate of a chemical reaction and experimental parameters 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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