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The bromination of acetone that occurs in acid solution is represented by this equation: CH₃COCH₃ (aq) + Br₂ (aq) → CH₃COCH₂Br (aq) + H⁺ (aq) + Br⁻ (aq) These kinetic data were obtained for given reaction concentrations. Initial Concentrations, M [CH₃COCH₃] | [Br₂] | [H⁺] 0.30 | 0.05 | 0.05 0.30 | 0.10 | 0.05 0.30 | 0.10 | 0.10 0.40 | 0.05 | 0.20 Initial rate, disappearance of Br₂, Ms⁻¹ 5.7 × 10⁻⁵ 5.7 × 10⁻⁵ 1.2 × 10⁻⁴ 3.1 × 10⁻⁴ Base on these data, the rate equations is:

1. Rate = k[CH₃COCH₃][H⁺]
2. Rate = k[CH₃COCH₃][Br₂]
3. Rate = k[CH₃COCH₃][Br₂][H⁺]²
4. Rate = k[CH₃COCH₃][Br₂][H⁺]

Correct answer: Rate = k[CH₃COCH₃][H⁺]

Solution

The rate is independent of [Br₂] as the rate remains constant when [Br₂] changes (compare rows 1 and 2). The rate depends on [H⁺] and [CH₃COCH₃] as it increases proportionally with their concentrations (compare rows 2 and 3, and rows 1 and 4). Thus, the rate law is Rate = k[CH₃COCH₃][H⁺].

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