If the $E_{cell}^0$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of ΔG0 and Keq?

For Competitive Exams

If the $E_{cell}^0$ for a given reaction has a negative value, which of the following gives the correct relationships for the values of ΔG⁰ and K_eq?

ΔG⁰ < 0; K_eq < 1

ΔG⁰ > 0; K_eq < 1

ΔG⁰ > 0; K_eq > 1

ΔG⁰ < 0; K_eq > 1

Explanation:

$E_{cell}^0$ < 0, so it is a non-spontaneous process

ΔG⁰ = – nFE⁰ = +ve, so ΔG⁰ > 0

ΔG⁰ = – 2.303RT log K

So, K < 1

Next Question

Which one of the following is incorrect for ideal solution?

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