For exothermic reaction, `E_a` (forward) -`E_a` (backward) is +ve /-ve.

What is exothermic reaction?

When the activation energies of the forward and backward reactions are equal, then :

k_(1) and k_(2) are the velocity constants of forward and backward reactions. The equilibrium constant K of the reaction is

What are exothermic reactions ? Give an example.

For an endothermic reaction, activation energy for the forward reaction is more/less than activation energy for the backward reaction.

An exothermic reaction is represented by the greph :

STATEMENT-1: The equilibrium constant of the exothermic reaction at high temperature decreases. STATEMENT-2: Since In (K_(2))/(K_(1))=(DeltaH^(@))/(R)[(1)/(T_(1))-(1)/(T_(2))] and for exothermic reaction , DeltaH^(@)= -ve and thereby, (K_(2))/(K_(1))lt1

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.5 KJ/mol , respectively . The reaction is: