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 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

The decomposition of N_2O_5 in carbon tetrachloride Solution has been found to be first order With respect to N_2O_5 with rate constant, k = 6.2 xx10^-4 s^-1 N_2O_5 (solution) rarr 2NO_2 (solution) +1//2 O_2 (g) Calculate the rate of the reaction when [N_2O_5]= 0.50 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?