Question

What is the difference between exergonic and exothermic? What is the difference between intermediate and transition state? What is the relation between activation energy and the rate of a reaction?

Answer 1

exothermic refers to change in enthalpy while exergonic refer to change in gibbs free energy. During the exergonic process, energy released which can be in the form of heat, light or sound.

During exothermic process, heat energy is released.

Internediate is a product formed which is intermediate between reactant and final products. While transition state is a formation of complex whose net rate is zero. Ther is no compound formation in case of transition state.

The rate constant is the rate at which the reaction takes place. Highe the rate constant, rapid is the reaction. It is the proportionality constant (K) defined as

-dCA/dt ( rate)= K*(CA)ⁿ, n = order of reaction and CA is concentration. It will have units of 1/time.(CA)^n-1. Where as activation energy is the energy required for formation of products. It is measued in J/mole. Lower the activation energy, the tendency to form products become more.