The rate constant k for the first order gas phase decomposition of ethyl iodide, C₂H₅I ⟶ C₂H₄ + HI is 1.60 x 10^-5 s^-1 at 600k and 6.36 x 10^-3 s^-1 at 700K. Calculate the energy of activation for this reaction.

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) 3NO_(g) ⟶ N₂O_(g) Rate = K[NO]²
(ii) H₂O_2(aq) + 3I^-_(aq) +2H⁺ ⟶ 2H₂O_(l) +I₃^- Rate = K[H₂O₂][I^-]
(iii) CH₃CHO_(g) ⟶ CH_4(g) + CO_(g) Rate = K[CH₃ CHO]^3/2
(iv) C₂H₅Cl_(g) ⟶ C₂H_2(g) + HCl_(g) Rate = K[C₂H₅Cl]²

A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
(i) doubled (ii) reduced to half

A reaction is first order in A and second order in B.
(i) Write the differential rate equation.
(ii) How is rate affected on increasing the concentration of B three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?

The rate constant for a first order reaction is 60 S^-1. How much time will it take to reduce the initial concentration of the reactant to its \({ \frac { 1 }{ 16 } }^{ th }\) value?