Gibbs free energy (ΔG) must be negative for a reaction to be:

A Endothermic

B Spontaneous (thermodynamically favorable)

C At equilibrium

D Endergonic

✓ Correct Answer: Option B

ΔG < 0: spontaneous (exergonic). ΔG = 0: equilibrium. ΔG > 0: non-spontaneous. ΔG = ΔH − TΔS.

💡 Why is B) the correct answer?

The correct answer to the question "Gibbs free energy (ΔG) must be negative for a reaction to be:" is Option B: Spontaneous (thermodynamically favorable).

The other options — A) Endothermic, C) At equilibrium, D) Endergonic — are incorrect for this Everyday Science question. As explained above: ΔG < 0: spontaneous (exergonic). ΔG = 0: equilibrium. ΔG > 0: non-spontaneous. ΔG = ΔH − TΔS.

📚 About This Everyday Science Practice Question

This 2-level Everyday Science question from the Chemistry - Elements & Compounds topic is part of One Paper Preparation's free exam preparation library. Each question includes the correct answer and a detailed explanation to help you understand the underlying concept, not just memorize the answer.

How to use this page: Read the question above, consider all four options (A through D), then check the highlighted correct answer and explanation. For active timed practice, start a free Everyday Science practice test or use flashcards for spaced repetition review.

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Gibbs free energy (ΔG) must be negative for a reaction to be:

✓ Correct Answer: Option B

📚 About This Everyday Science Practice Question

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