The rate constant of a reaction at `500^@C` is `1.6xx10^3 M^(-1)s^(-1)`. What is the frequency factor of the reaction if its activation energy is `56 kJmol^(-1)`. `(9.72 xx106 M^(-1)s^(-1))`

The rate constant of a reaction is 2.1 xx 10^(-2) litre mol^(-1)s^(-1) . The order of reaction is

The rate constant of a certain first order reaction is 3.12xx10^(-3) min^(-1) What is the molarity of the reactant after 1.5 hours , If initial concentration is 0.045 M ?

The rate constants for a first order reaction are 0.6 s^(-1) at 313 K and 0.045 s^(-1) at 293 K. What is the activation energy?

The rate constant of a first order reaction at 25^@C is 0.24 s^(-1) . If the energy of activation of the reaction is 88 kJ mol^(-1) , at what temperature would this reaction have rate constant of 4 xx 10^(-2) s^(-1) ?

For a reaction A+2B rarr C , the rate law is, rate= kxx[A]xx[B]^2 . If the rate constant of the reaction is 3.74xx10^(-2) M^(-2)s^(-1) , calculate the rate of the reaction when the concentrations of A and B are 0.126 M and 0.142 M respectively.

The rate law for the reaction A+B rarr C is found to be rate = k [A]^2 [B] . The rate constant of the reaction at 25^@C is 6.25 M^(-2)S^(-1) . What is the rate of reaction, When [A] = 0.1 mol.dm^(-3) and [B] = 0.2 mol.dm^(-3) ?