The decomposition of `H_2 O_2`, in the presence of Iodide ion has been found to be first order in `H_2 O_2` .
The rate constant has been found to be `1.01xx10^-2 min^-1`. What concentration of `H_2 O_2` would give rate of `1.12 xx 10^-2 mol L^-1 min^-1?

Explanation

`2H_2O_2(aq) overset(1(aq))(rarr)2H_2O(l)+O_2(g)`
Rate=`k[H_2O_2]`
`r=(1.01xx10^(-2)min^(-1))[H_2O_2]`
`(becausek=1.01xx10^(-2)min^(-1))`
(i) Rate, r=?,`[H_2O_2]=0.4" mol L"^(-1)`
`r=(1.01xx10^(-2)" min"^(-1))xx(0.4" mol L"^(-1))`
`=4.04xx10^(-3)" mol L"^(-1)min^(-1)`
(ii) `[H_2O_2]=1/2xx0.4" mol L"^(-1)`
=0.2 mol `L^(-1)`
r=`(1.01xx10^(-2)min^(-1))xx(0.2xx" mol L"^(-1))`
`=2.02xx10^(-3)" mol L"^(-1)min^(-1)`