If ΔG < 0 at a given temperature, which statement about the equilibrium constant K is true?

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Prepare for the NANTeL Chemistry Certification and Engineering Fundamentals Test with multiple choice questions, detailed explanations, and key insights to boost your understanding and confidence. Ace your exam!

Multiple Choice

If ΔG < 0 at a given temperature, which statement about the equilibrium constant K is true?

Explanation:
The main idea is how Gibbs free energy relates to how far a reaction goes toward products at a given temperature. The standard relation is ΔG° = -RT ln K, which can be rearranged to K = e^{-ΔG°/(RT)}. If ΔG° (or the context equivalent to standard conditions) is negative, the exponent is positive, so K must be greater than 1. That means the equilibrium lies to the right, with more products than reactants at equilibrium. So a negative free-energy change corresponds to an equilibrium constant greater than one.

The main idea is how Gibbs free energy relates to how far a reaction goes toward products at a given temperature. The standard relation is ΔG° = -RT ln K, which can be rearranged to K = e^{-ΔG°/(RT)}. If ΔG° (or the context equivalent to standard conditions) is negative, the exponent is positive, so K must be greater than 1. That means the equilibrium lies to the right, with more products than reactants at equilibrium. So a negative free-energy change corresponds to an equilibrium constant greater than one.

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