5. (a) First-class reaction N.OF (g) → 2NO2 (g) +1/202 (g) The initial concentration of N, 05 at 318 K was 1.24 x 10-2 mol L-1, which is 60 minutes Then calculate the velocity constant at 318 K remaining 0.20x10-2 mol L-1. 4

The initial concentration of the first order reaction, N_2O_(5(g))to2NO_(2(g))+1/2O_(2(g)) was 1.24xx10^(-2)molL^(-1) .The concentration of N2O5 after ‘1’ hour was 0.20 x 10-2 mol L-1 Calculate the rate constant of the reaction at 300 K.

The initial concentration of N_2 O_5 in the following first order reaction, N_2 O_5 (g) to 2NO_2 (g) + 1/2 O_2 (g) was 1.24 xx 10^(-2) mol L^(-1) at 318 K. The concentration of N_2 O_5 after 60 minutes was 0.20 xx 10^(-2) mol L^(-1) . Calculate the rate constant of the reaction at 318 K.

The initial concentration of N_(2)O_(5) in the following first order reaction: N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g) was 1.24 xx 10^(-2) mol L^(-1) at 318 K . The concentration of N_(2)O_(5) after 60 min was 0.20 xx 10^(-2) mol L^(-1) . Calculate the rate constant of the reaction at 318 K .

The initial concentration of N_(2)O_(5) in the following first order reaction N_(2)O_(5)(g) to 2NO_(2)(g) + (1)/(2) O_(2)(g) was 1.24 xx 10^(-2) mol L^(-1) at 318K. The concentration of N_(2)O_(5) after 60 mintues was 0.2 xx10^(-2) mol L^(-1) . Calculate the rate constant of the reaction.