Among the two reactions, one with K eq =1000 and other with K eq =0.001, which is likely to be more exergonic is to be stated. Concept introduction: When ΔG 0 is negative, the reaction is exergonic, has a favorable equilibrium constant and occurs spontaneously. When ΔG 0 is positive, the reaction is endergonic, has an unfavorable equilibrium constant and cannot occur spontaneously. To state: Among the two reactions, one with K eq =1000 and other with K eq =0.001, which is likely to be more exergonic.

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Chapter 6.7, Problem 11P

Interpretation Introduction

Interpretation:

Among the two reactions, one with K_eq=1000 and other with K_eq=0.001, which is likely to be more exergonic is to be stated.

Concept introduction:

When ΔG⁰ is negative, the reaction is exergonic, has a favorable equilibrium constant and occurs spontaneously. When ΔG⁰ is positive, the reaction is endergonic, has an unfavorable equilibrium constant and cannot occur spontaneously.

To state:

Among the two reactions, one with K_eq=1000 and other with K_eq=0.001, which is likely to be more exergonic.

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