For a reaction, rate constant is \(ln2s^{-1}\) at temperature "300K" .If activation energy of this reaction is 600R In 10 ,then calculate half life (approx.) of this reaction at temperature "600K"

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))

The activation energy of a reaction is zero. Its rate constant at 280 K is 16 xx 10^(-6) s^(-1) the rate constant at 300k is

Calculate the activation energy of a reaction whose reaction rate at 310 K gets doubled for 320 K rise in temperature.

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 ?

A first order reaction has a rate constant, k = 5.5 xx 10^(-14) s^(-1) , calculate the half life of reaction.

Calculate the activation energy of a reaction whose reaction rate at 300 K double for 10 K rise in temperature.

(a) Explain the following terms : (i) Order of a reaction (ii) Molecularity of a reaction (b) The rate of a reaction increases four times when the temperature changes from 300 K to 320 K. Calculate the energy of activation of the reaction, assuming that it does not change with temperature. (R = 8.314 J K^(-1) mol^(-1))