Energy of reaction#!#Arrhenious equation

The activation energy of reaction is equal to

Rate constant k of a reaction varies with temperature according to the equation logk = constant -E_a/(2.303R)(1/T) where E_a is the energy of activation for the reaction . When a graph is plotted for log k versus 1/T , a straight line with a slope - 6670 K is obtained. Calculate the energy of activation for this reaction

The activation energy of a reaction is zero. The rate constant of the reaction

The activation energy of a reaction is zero. The rate constant of this reaction

The equilibrium constant of a reaction and the standard Gibbs energy change of the reaction are related by the equation