For a first order reaction `t_(0.75)` is `1386 s`. Therefore, the specific rate constant is

Options

A. `10^(-1) s^(-1)`
B. `10^(-3) s^(-1)`
C. `10^(-2) s^(-1)`
D. `10^(-4) s^(-1)`

Answer

B

Explanation

`t_(0.75) =2t_(1//2)`
`:. t_(1//2) = (1386)/(2) =693 s`
`k = (0.693)/(693s) = 10^(-3) s^(-1)`