Rate law for the reation `A + B to ` product is rate = `k [A]^(2) [B]` . What is the rate constant , if rate of reaction at a given temperature is `0.22 Ms^(-1)` , when [A] = 1M and [B] = 0.25 M ?

Options

A. `3.52 M^(-2) s^(-1)`
B. `0.88 M^(-2) s^(-1)`
C. `1.136 M^(-2) s^(-1)`
D. `0.05 M^(-2) s^(-1)`

Answer

B

Explanation

For reaction , ` A + B to `product
`(dx)/(dt) = k[A]^(2) [ B] implies 0.22 = k(1)^(2) (0.25)`
`therefore k = (0.22)/(0.25) = 0.88 M^(-2) s^(-1)`