Question

A redox reaction has an equilibrium constant of K=0.055. What is true of ΔG∘rxn and E∘cell for this reaction?

choices:

E∘cell is positive and ΔG∘rxn is negative
E∘cell is negative and ΔG∘rxn is positive
E∘cell is negative and ΔG∘rxn is negative
E∘cell is positive and ΔG∘rxn is positive
Can you please explain the problem?

Answer 1

In a redox reaction with a equilibrium constant (K) of 0.055, the ΔG∘rxn is positive and the E∘cell is negative.

Step-by-step explanation:

In a redox reaction, the equilibrium constant (K) is related to the standard cell potential (E∘cell) and the standard Gibbs free energy change (ΔG∘rxn). Based on the information provided, K=0.055, which is less than 1. This indicates that the reaction favors the reactant side at equilibrium.

Since the value of K is less than 1, the value of ΔG∘rxn will be positive. This means that the reaction is not spontaneous under standard conditions and requires an input of energy to proceed in the forward direction. As a result, E∘cell will also be negative.

Therefore, the correct answer is: E∘cell is negative and ΔG∘rxn is positive.