JEE Chemistry 2024 Question with Solution

Given: The statements relate the sign of $\Delta G$ to spontaneity and reversibility.

Find: Which statement is not correct.

For thermodynamic processes:

for a spontaneous reaction,

for a reversible reaction at equilibrium, and

for a non-spontaneous reaction.

Now compare each option:

1. $\Delta G$ is negative for a spontaneous reaction — correct.
2. $\Delta G$ is positive for a spontaneous reaction — incorrect.
3. $\Delta G$ is zero for a reversible reaction — correct.
4. $\Delta G$ is positive for a non-spontaneous reaction — correct.

The solution marks The Correct Option is B. The remaining solution text appears unrelated to this thermodynamics question, so the answer is taken from the explicit conclusion in the solution.

Therefore, the correct option is B.

Given: A question on Gibbs free energy and reaction spontaneity.

Find: The incorrect statement.

Use the standard criteria:

• Spontaneous process: $\Delta G < 0$
• Reversible equilibrium condition: $\Delta G = 0$
• Non-spontaneous process: $\Delta G > 0$

Hence the statement assigning positive $\Delta G$ to a spontaneous reaction contradicts thermodynamics.

Therefore, the incorrect statement is $\Delta G$ is positive for a spontaneous reaction, so the correct option is B.