The decomposition of `N_2O_5` at 318 K according to the following equation follows first order reaction: `N_2O_5(g) rarr 2NO_2(g) + 1/2 O_2(g)` The initial concentration of `N_2O_5` was `1.24 xx 10^-2 mol L^-1` and that after 60 minutes was `0.20 xx 10^-2 mol L^-1` . Calculate the rate constant of the reaction at 318 K.

For the first order reaction 2N_2O_5 (g) rarr 4 NO_2(g)+ O_2(g) which is incorrect:-

The initial concentration of N_2O_5 in the following first order reaction N_2O_5(g) rarr 2 NO_2(g) + 1/2O_2 (g) was 1.24 x 10^(-2) mol L^(-1) Calculated the rate constant of the reaction at 318 K.

The rate of a reaction is 1.209 xx10^-4L^2 mol^-2 s^-1 . The order of the reaction is :

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^-4s^-1 N_2 O_5(G)rarr2NO_2(g)+1/2O_2(g) What concentration of N_2 O_5 would give a rate of 4.2xx10^-3 mol L^-1 s^-1 ?

For the reaction N_2O_5(g)rarr 2NO_2(g) + 1/2 O_2 (g) the value of rate of disappearance of N_2O_5 is given as 6.25 xx 10^-3 mol L^-1 s^-1 . The rate of formation of NO_2 and O_2 is given respectively as :

The decomposition of N_2O_5 in CC1_4 at 318K has been studied by monitoring the concentration of N_2O_5 in the solution. Initially the concentration of N_2O_5 is 2.33 mol L^(-1) and after 184 minutes, it is reduced to 2.08 mol L^(-1) . The reaction takes place according to the equation 2 N_2O_5 (g) rarr 4 NO_2 (g) + O_2 (g) Calculate the average rate of this reaction in terms of hours, minutes and seconds. What is the rate of production of NO_2 during this period?

The reaction - N_2O_5 (i n C Cl_4) rarr 2NO_2+1/2 O_2 (g) is first order in N_2O_5 with rate constant 6.2xx10^-4 s^-1 . What is the value of rate of reaction when [N_2O_5] = 1.25 mol L^-1 ?

The rate of a first order reaction is 1.8 xx10^-3 mol L^-1 mi n^-1 when the initial concentration is 0.3 mol L^-1 . The rate constant in the units of second is :

The following data were obtained for the reaction: 2NO_2(g)+F_2(g) rarr 2NO_2F Determine: rate of reaction when [NO_2] = 0.50 mol L^-1 and [F_2] = 0.60 mol L^-1 .