The rate constant for the decompoistion of a certain reaction is described by the equation:
`log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T)`
Energy of activation (in `kcal`) is

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) At what temperature, rate constant is equal to pre-exponential factor?

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) At what temperature, rate constant is equal to pre-exponential factor?

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) Pre-exponential factor for this reaction is

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) Pre-exponential factor for this reaction is

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) What is the effect on the rate of reaction at 127^(@)C , if in the presence of catalyst, energy of activation is lowered by 10 kJ mol^(-1) ?

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) What is the effect on the rate of reaction at 127^(@)C , if in the presence of catalyst, energy of activation is lowered by 10 kJ mol^(-1) ?

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) A two-step mechanism has been suggested for the reaction of nitric oxide and bromine: NO(g) + Br_(2)(g) overset(k_(1))rarr NOBr_(2)(g) NOBr_(2)(g)+NO(g) overset(k_(2))rarr 2NOBr(g) The observed rate law is, rate = k[NO]^(2)[Br_(2)] . Hence, the rate-determining step is

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) A two-step mechanism has been suggested for the reaction of nitric oxide and bromine: NO(g) + Br_(2)(g) overset(k_(1))rarr NOBr_(2)(g) NOBr_(2)(g)+NO(g) overset(k_(2))rarr 2NOBr(g) The observed rate law is, rate = k[NO]^(2)[Br_(2)] . Hence, the rate-determining step is

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 ?