The rate constant for the decomposition of hydrocarbons is `2.418 xx 10^(-5)s^(-1)` at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.

The first order rate constant for the decomposition of ethyl iodide by the reaction C_2H_5I(g) rarr C_2H_4 (g) + HI(g) at 600K is 1.60 x 10^(-5) s^(-1) . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700K.

The rate constant for the decomposition of N_2O_6 , N_2O_6 rarr N_2O_4+1/2O_2 is 3.46 xx 10^(-5) at 25^@ C and 4.87 xx 10^(-3) at 65^@ C. Calculate the energy of activation of the reaction.

The value of k for a reaction is 2.96 xx 10^(-30)s^(-1) . What is the order of reaction ?

The rate constant for a reaction is found to be 1.96xx10^-2 s^-1 at 313K. The activation energy of the reaction is 93.62 kJ mol^-1 . Calculate the frequency factor ,A.

The rate constant of a reaction is 1.2 xx10^-3 sec^-1 at 30^@C and 2.1xx10^-3 sec^-1 at 40^@C . Calculate the energy of activation of the reaction.

The rate constant of a reaction is 1.2 xx10^(-5) mol^(-2)"litre"^(2)s^(-1) . The order of the reaction is:

The decomposition of A into product has value of k as 4.5 xx 10^3 s^-1 at 10°C and energy of activation 60 kJ mol^-1 . At what temperature would k be 1.5 xx 10^4 s^-1 ?

The rate constant of a reaction is 1.5 xx 10^7 sec^(-1) at 50^@ C and 4.5 xx 10^7 sec^(-1) at 100^@ C . Calculate energy of the activation for the reaction.

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

The value of decay constant of Co^(60) is 2.5xx 10^(-7)"min"^(-1) . The activity of 2.0 g of the sample is nearly :