Chemistry

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Chemistry HELP - Rates of reaction, redox reactions? 10 points?
An structural isomer of bromobutane (C4H9Br) can be hydrolysed using aqueous sodium hydroxide to produce butanol. This can be represented by the following equation:

C4H9Br(l) + OH-(aq) > C4H9OH(l) + Br-(aq)

This reaction was investigated experimentally and the following results
were obtained:

Experiment A -
Initial [bromobutane], mol dm-3 = 0.01
Initial [OH-], mol dm-3 = 0.01
Initial rate, mol dm-3s-1 = 4.3 x 10 -4^

Experiment B
Initial [bromobutane], mol dm-3 = 0.01
Initial [OH-], mol dm-3 = 0.02
Initial rate, mol dm-3s-1 = 8.6 x 10-4^

Experiment C -
Initial [bromobutane], mol dm-3 = 0.02
Initial [OH-], mol dm-3 = 0.02
Initial rate, mol dm-3s-1 = 1.7 x 10-3^

(b) (i) Deduce the overall order of the reaction and write the rate equation for this reaction

(ii) What is meant by the rate-limiting step of a reaction mechanism?

(iii) What can you say about the rate-limiting step for the above reaction?

(iv) Suggest which isomer of bromobutane is likely to react via this rate-limiting step. Explain your answer fully.

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