Question

If $G$ represents Gibbs free energy, select the correct statement(s).

• A. If $\Delta G = 0$, reaction will proceed only in one direction
• B. If $\Delta G = 0$, reaction will be in equilibrium
• C. If $\Delta G<0$, reaction will proceed forward
• D. If $\Delta G>0$, reaction will not proceed forward

Hint:

Remember: $\Delta G = 0$ → equilibrium, $\Delta G<0$ → spontaneous, $\Delta G>0$ → non-spontaneous.

Answer 1

The Correct Option is B, C, D

Gibbs free energy determines the spontaneity of chemical reactions under constant pressure and temperature.
Step 1: Interpret ΔG.
- If $\Delta G = 0$, the reaction is at equilibrium; forward and backward rates are equal. - If $\Delta G<0$, the reaction is spontaneous in the forward direction. - If $\Delta G>0$, the forward reaction is non-spontaneous.
Step 2: Evaluate given statements.
(A) Incorrect — $\Delta G = 0$ does \textit{not} imply one-direction movement; it implies no net reaction.
(B) Correct — equilibrium condition.
(C) Correct — negative ΔG means spontaneous forward reaction.
(D) Correct — positive ΔG means the reaction will not proceed forward spontaneously.
Thus, the correct statements are (B), (C), and (D).
Final Answer: (B), (C), (D)