Question

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.
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Initial Initial rate,
Concentrations, M disappearance of
Br₂, Ms⁻¹
[CH₃ COCH₃] [Br₂] [H⁺]
0.30 0.05 0.05 5.7×10⁻⁵
0.30 0.10 0.05 5.7 × 10⁻⁵
0.30 0.10 0.10 1.2 × 10⁻⁴
0.40 0.05 0.20 3.1 × 10⁻⁴
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Based on given data, the rate equations is:
(a) Rate = k[CH₃COCH₃][H⁺]
(b) Rate = k [CH₃COCH₃][Br₂]
(c) Rate = k [CH₃COCH₃] [Br₂] [H⁺]²
(d) Rate = k [CH₃COCH₃][Br₂] [H⁺]

Answer 1

Explanation:

c) Rate = k [CH₃COCH₃] [Br₂] [H⁺]² is your answer g

Answer 2

The rate equations is:

• Equation : CH₃COCH₃ (aq) + Br₂ (aq) → CH₃COCH₂Br (aq) + H⁺(aq) + Br⁻ (aq)

• Let us observe kinetic data given for reaction.

1) Rate= 5.7×10⁻⁵ when [CH₃ COCH₃] = 0.30,[Br₂] = 0.05, [H⁺] = 0.05

2) When concentration of [Br₂] is doubled, there is no change on rate i.e rate is independent of concentration of [Br₂].

• By using elimination method for choosing correct option, there is only one option in which rate is independent of concentration of [Br₂] i.e optio (a)

• Hence correct answer is (a)

Rate = k[CH₃COCH₃][H⁺]