Answer: 1/[A] = 1/[A]₀ + kt.
- A ln[A] = ln[A]₀ - kt
- B 1/[A] = 1/[A]₀ + kt
- C [A] = [A]₀e<sup>-kt</sup>
- D 1/[A] = 1/[A]₀ - kt
Correct answer: B. 1/[A] = 1/[A]₀ + kt
Explanation: For second-order: 1/[A] = 1/[A]₀ + kt. A plot of 1/[A] vs time gives a straight line with slope k.
First-order decay curve: concentration halves every t½, and that half-life is constant - a defining test for first-order kinetics.
Concept context
Study the speed of reactions and what affects it: concentration, temperature, and catalysts. Covers rate law, order of reaction, the Arrhenius equation, and reaction mechanisms step by step.