1. Δ G^° > 0 ; K_eq > 1 2. Δ G^° 1 3. Δ G^° 0 ; K_eq < 1

If the E^°_cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of Δ G^° and K_eq?

1. \(\Delta G^\circ > 0\); \(K_{eq} > 1\)

2. \(\Delta G^\circ < 0\); \(K_{eq} > 1\)

3. \(\Delta G^\circ < 0\); \(K_{eq} < 1\)

4. \(\Delta G^\circ > 0\); \(K_{eq} < 1\)

Doubtly Asked 30 Oct 2026 NEET UG 2016 Phase 2 Practice test neet Save WhatsApp Report

Best answer

Answer: 4. \(\Delta G^\circ > 0\); \(K_{eq} < 1\)

Key idea: \(\Delta G^\circ=-nFE^\circ_{cell}=-RT\ln K\).

If \(E^\circ_{cell}<0\), then \(\Delta G^\circ>0\), so \(\ln K<0\) and \(K_{eq}<1\). The reaction is non-spontaneous under standard conditions.

Doubtly AI · 30 Oct 2026 AI-generated · not yet verified Report

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