Justify the following statements : (a) Reaction with ΔG° < 0 always

1.	Justify the following statements : (a) Reaction with ΔG° < 0 always have an equilibrium constant greater than. (b) Many thermodynamically feasible reaction do not occur under ordinary conditions. (c) At low temperatures enthalpy change dominates the AG expression and at high temperature, it is the entropy which dominates the value of AG.
Answer» (a) ΔG° = -2.303 RT logK If K > 1, ΔG° will be less than zero because products formed are more than that of reactants, i.e., process is spontaneous in forward direction. (b) It is because heat energy is required to overcome activation energy. (c) ΔG = ΔH - TΔS, At low temperatures ΔH > TΔS whereas at high temperature TΔS >ΔH ∴ ΔG decreases, i.e., becomes negative.

Justify the following statements : (a) Reaction with ΔG° < 0 always have an equilibrium constant greater than. (b) Many thermodynamically feasible reaction do not occur under ordinary conditions. (c) At low temperatures enthalpy change dominates the AG expression and at high temperature, it is the entropy which dominates the value of AG.

Answer»

(a) ΔG° = -2.303 RT logK If K > 1, ΔG° will be less than zero because products formed are more than that of reactants, i.e., process is spontaneous in forward direction.

(b) It is because heat energy is required to overcome activation energy.

∴ ΔG decreases, i.e., becomes negative.

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