Given that the Arrhenius factor (A)" for a desorption is equal to \(10^{13}s^{-1}\) at "300K" .Calculate half life time for desorption if desorption activation energy is "10kJ/mol"

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

The activation energy for the decomposition of hydrogen iodide at 581 K is 209.5 kJ mol^(–1) . Calculate the fraction of molecules having energy equal to activation energy.

The time required for 10% completion of a first order reaction at 298 K is equal to that required for its 25% completion at 308 K . If the pre-exponential factor for the reaction is 3.56 xx 10^(9) s^(-1) , calculate its rate constant at 318 K and also the energy of activation.

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"

If the half-lives of the first order reaction at 350 K and 300 K are 2 and 20 seconds respectively, the activation energy of the reaction in kJ "mol"^(-1) is :