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.

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

The molecularity of the reaction 2NO+O_2 rarr 2 NO_2 is,

Balance the following chemical equation: Pb(NO_3)_2(s) rarr 2PbO(s)+NO_2(g)+O_2(g)

The following rate data were obtained for the reaction : 2NO(g) + O_2(g) rarr 2 NO_2 (g) Determine the rate law expression and order of the reaction.

Write the equilibrium constant expression for the following reactions. CH_(4)(g) + 2O_(2)(g) hArr CO_(2)(g) + 2H_(2)O(l)

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?

For the reaction : 2N_2O_5 rarr 4NO_2+O_2 the rate of reaction measured as (Delta[NO_2])/(Deltat) was found to be 4 xx 10^(-3)" mol L"^(-1) is s^(-1) . Calculate the rate of reaction, expressed in terms of N_2O_5