For the reaction

`k_(1) = 1.78 xx 10^(-3)s^(-1)` and `k_(2) = 5.8 xx 10^(-5)s^(-1)` for the initial concentration of `[Cr(H_(2)O)_(4)Cl_(2)]^(o+)` is `0.0174 mol L^(-)` at `0^(@)C`. Calculate the value of time at which the concentration of `[Cr(H_(2)O)_(5)Cl]^(2+)` is maximum.

Explanation

The time required for two consecutive reactions to react its maximum activity or concentration is given by
`t - (2.303(logk_(1)-logk_(2)))/(k_(1) - k_(2))`
`= (2.303(log 1.78 xx 10^(-3) - log 5.8 xx 10^(-5)))/(1.78 xx 10^(-3) - 5.8 xx 10^(-5))`
`= 1990 s`.