1-Bromobutane reacts with water to form 1-butanol according to the following equation overall rate law for this proposed mechanism is rate = k [C₄H₉Br]
The reaction intermediate in the chemical species that is formed in one elementary step and consumed in subsequent step and the slowest step in the reaction mechanism is rate determining step and the rate determining step limit the overall rate and therefore determines the rate law for the overall reaction
Here given reaction
C₄H₉Br(aq) + 2H₂O(l) → C₄H₉OH(aq) + H₃O⁺(aq) + Br⁻(aq)
And the following is a proposed mechanism for the reaction
C₄H₉Br(aq) → C₄H₉⁺(aq) + Br⁻(aq) slow
C₄H₉⁺(aq) + H₂O(l) → C₄H₉OH₂⁺(aq) fast
C₄H₉OH₂⁺(aq) + H₂O(l) → C₄H₉OH(aq) + H₃O⁺(aq) fast
So in that 1st step is the rate determining step means slow step
So rate expressions take the general form: rate = k . [A]a . [B]b
So given equation rate expressions is k [C₄H₉Br]
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