The rate constant for a first order decomposition reaction is given by "log K=\(10-\frac{1000}{T}\) .Then,what will be activation energy in kcal/mol?

The rate constant for a first order decomposition reaction is given by log K=10 - 1000/T .Then,what will be activation energy in kcal/mol?

The rate constant 'K' for pseudo first order reaction is

The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate the activation energy for the reaction [R=8.314JK^(-1)mol^(-1)]

The rate constant for the first order decompoistion of a certain reaction is described by the equation log k (s^(-1)) = 14.34 - (1.25 xx 10^(4)K)/(T) (a) What is the energy of activation for the reaction? (b) At what temperature will its half-life periof be 256 min ?

The rate constant for a first order reaction becomes six times when the temperature is raised from 350 to 400 K. Calculate the energy of activation for the reactions.

The rate constant of a first order reaction are 0.58 s^(-1) at 313 K and 0.045 s^(-1) at 293 K. what is the energy of activation for the reaction?

The activation energy of a first order reaction at 300 K is 60 kJ "mol"^(-1) . In the presence of a catalyst, the activation energy is lowered to 50 kJ "mol"^(-1) at the same teperature. How many times the rate of reaction will change ?

For a first order reactin, rate constant is given is log k = 14 - (1.2 xx 10^(4))/(T) , then what will be value of temperature if its half life period is 6.93 xx 10^(-3) min ?