The decomposition of hydrogen peroxide in the presence of iodide ion has been found to be first order in `H_2O_2`:
`2H_2O_2 (aq) overset(1^(-)(aq))(rarr) 2H_2O(l) + O_2 (g)`.
The rate constant has been found to be `1.01 xx10^(-2) " min"^(-1)` :
(a) Calculate the rate of reaction when `[H_2O_2] = 0.4" mol lit"^(-1)`.
(b) What concentration of `[H_2O_2]` would give a rate of `1.12 xx 10^(-2)" mol lit"^(-1)" min"^(-1)` ?

Explanation

`2H_2O_2 overset(I^(-))(rarr)2H_2O + O_2`
(i) Rate Expration = `k [H_2O_2]`
=` 1.01 xx 10^(-2) "min"^(-1) xx 0.4 "mol" l^(-1)`
`= 4.04 xx 10^(-3) mol^(1) "min"^(-1)`