The value of rate constant for the decomposition of nitrogen peroxide, `N_{2}O_{5}rarrN_{2}O_{4}+1/2O_{2}` is `3.46*10^-5` at 25 degree celcius and` 4.87*10^-3 at 65 degree celcius. Calculate the énergy of activation for the reaction. (R=8.314] (k)^(-1) (mol)^(-1)

Which of the following oxides of nitrogen is solid NO_2 N_2 O N_2 O_3 N_2 O_5

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 rate constant for the decomposition of hydrocarbons is 2.418 x 10^(-5) (s)^(-1) at 546 (~K) . if the energy of activation is 179.9 (kJ) / (mol) , what wilt be the value of pre-exponential factor:

The rate constant for the reaction, 2N_(2)O_(5) rarr 4NO_(2) +O_(2) is 3.0 xx10^(-5) s^(-1) If the rate is 2.40 xx10^(-5) mo L^(-1) S^(-1) then the concentration of N_(2)O_(5) (in mo L^(-1) ) is

For the reaction, 2N_{2}O_{5}(g)harr4NO_{2}(g)+O_{2}(g) . If the concentration of NO_{2} increases by 3.0xx10^-3 molL^-1 in six seconds then what is the rate of reaction?

The temperature dependence of the rate of a chemical reaction can be explained by Arrhenius equation.The rate of a chemical reaction doubles for an increase of 10 K in absolute temperature from 300 K. Calculate the activation energy(Ea)? [ R=8.314 JK^(-1)mol^(-1),log 2 = 0.3010 ].