The reaction AK−→Product, is a zero order while the reaction BK−→Product, is a first order reaction. For what initial concentration of 'A' are the half lives of the two reactions equal? (Rate constant values are the same for both the reactions)
A
(loge4)M
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B
2M
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C
log2M
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D
ln2M
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Solution
The correct option is A(loge4)M For a zero order reaction, a=kt ∴a2=k×t(12), From the second reaction, which has an order of 1, t(12)=loge2k ⇒a=2ln2=loge4 M