The decomposition of hydrogen peroxide has been found to be first order
The rate constant has beem found to be `1.01xx10^-2 min^-1` . Calculate the rate of reaction when `[H_2 O_2]=0.4 mol L^-1`

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?

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) ?

The rate constant of a reaction is 3xx10^2 mi n^-1 . What is the order of reaction ?

The decomposition of N_2 O_5 in carbon tetrachloride solution has been found to be first order with respect to N_2 O_5 with rate constant, k-6.2xx10^-4s6-1 N_2 O_5(G)rarr2NO_2(g)+1/2O_2(g) Calculate the rate of reaction when [N_2 O_5]=2.50mol L^-1