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The decomposition of hydrogen peroxide i...

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)` ?

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The decomposition of hydrogen peroxide in the presence of iodide ion has been found to be first order with respect to H_2O_2 with rate constant k is 1.01 xx 10^(-2) min^(-1) . Calculate the rate of reaction when [H_2O_2] = 0.15 mol L^(-1)

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?