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The rate of first-order reaction is 1.5 ...

The rate of first-order reaction is `1.5 xx 10^(-2) M "min"^(-1)` at `0.5 M` concentration of reactant. The half-life of reaction is

A

0.383 min

B

23.1 min

C

8.73 min

D

7.53 min

Text Solution

Verified by Experts

rate `=k[A]^1`
`k = (1.5xx 10^(-2))/0.5 mi n^(-1)`
`:.t_(1//2) = 0.693/k = (0.693)/(1.5xx 10^(-2))= 23.1 min`
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