Choose the Incorrect Statement:

Correct option is C

The incorrect statement is (c). Gibbs's free energy change (ΔG) must be negative for a reaction to occur spontaneously, not positive. If ΔG is positive, the reaction is non-spontaneous, meaning it requires an input of energy to proceed.
Explanation of Other Options:
1. (a) For a system at equilibrium, chemical potential is the same in all phases:
· Correct. At equilibrium, the chemical potential of a substance must be the same across all phases for no net change to occur.
2. (b) Gibbs's free energy change is zero at the equilibrium state of a system:
· Correct. At equilibrium, ΔG=0, meaning there is no driving force for the reaction to move forward or backward.
3. (d) ΔG\Delta GΔG will become more negative with increasing temperature:
· Correct. Depending on the enthalpy (ΔH) and entropy (ΔS) terms, increasing temperature can make ΔG more negative if the entropy change (ΔS) is positive.
Information Booster: 1. Gibbs Free Energy (ΔG): Determines the spontaneity of a reaction:
· ΔG<0: Reaction is spontaneous.
· G>0: Reaction is non-spontaneous.
· ΔG=0: Reaction is at equilibrium.
2. Equation for ΔG\Delta GΔG:
ΔG=ΔH−TΔS
Where:
· ΔH = Enthalpy change
· T = Temperature (in Kelvin)
· ΔS = Entropy change
3. Chemical Potential: Represents the free energy per mole of a substance and must be equal in all phases at equilibrium.
4. Temperature Dependence: If ΔS is positive, increasing temperature makes ΔG more negative, favoring spontaneity.
5. Equilibrium: A state where the forward and reverse reactions occur at the same rate, and no net change is observed.
Additional Knowledge: · Spontaneous Reactions: Occur without external energy input and have ΔG<0.
· Non-Spontaneous Reactions: Require energy input and have ΔG>0.
· Effect of Temperature: High temperatures favor reactions with positive ΔS.
· Phase Equilibrium: Chemical potential equality ensures no net transfer of matter between phases.