for a reaction, rate constant is ln2 `s^(-1)` at temperature 300k. if activation energy of this reaction is 600Rln10 then calculate half life of this reaction at 600k

The activation energy of a reaction is zero. The rate constant of this reaction

For a reaction, the rate constant is 2.34 s^(-1) . The half-life period for the reaction is

The activation energy of a reaction is zero. Will the rate constant of the reaction depend upon temperature ?

For a reaction, the rate constant is expressed as k = Ae^(-40000//T) . The energy of the activation is

A reaction is carried out at 600 K . If the same reaction is carried out in the presence of catalyst at the same rate and same frequency factor, the temperature required is 500 K . What is the activation energy of the reaction, if the catalyst lowers the activation energy barrier by 20 KJ//mol ?

The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is : ( Assume Activation energy and pre-exponential factor are independent of temperature, ln(2) = 0.693, R = 8.314J - mol^(-1) K^(-1))

In a first order reaction A to B, if k is rate constant and initial concentration of the reactant A is 2 M then the half life of the reaction is:

The rate constant of a first order reaction is 10^(-3) m i n^(-1) at 300K . The temperature coefficient of the reaction is 2. What is the rate constant of the reaction at 350K approximately ?