The catalytic decomposition of `H_(2)O_(2)` was studied by titrating it at different intervals with `KMnO_(4)` solution.Calcualte the rate constant from the following data assuming the reaction to be of the first order
time t(seconds): 0 600 1200
`KMnO_(4)` (mL) :22.8 13.8 8.2

Explanation

First order reaction `k=(1)/(t) lm(a)/(a-x)`
for t =1200 s `k=(1)/(1200 s) ln (22.8)/(8.2) =(1)/(1200 s) ln 2.7805 =8.522 xx10^(-4) s^(-1)`
Values of k are nearly constant indicating that the reaction is first order