What is the relationship between Gibbs free energy (ΔG) and cell potential (E) i

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Question: What is the relationship between Gibbs free energy (ΔG) and cell potential (E) in an electrochemical cell?

Options:

Correct Answer: ΔG = -nFE

Solution:

The relationship is given by ΔG = -nFE, where n is the number of moles of electrons and F is Faraday\'s constant.

What is the relationship between Gibbs free energy (ΔG) and cell potential (E) in an electrochemical cell?

What is the relationship between Gibbs free energy (ΔG) and cell potential (E) in an electrochemical cell?

Step 1: Understand that Gibbs free energy (ΔG) is a measure of the energy available to do work in a chemical reaction.
Step 2: Know that cell potential (E) is the voltage produced by an electrochemical cell during a reaction.
Step 3: Recognize that there is a mathematical relationship between ΔG and E, which is expressed as ΔG = -nFE.
Step 4: Identify the variables in the equation: n is the number of moles of electrons transferred in the reaction, and F is Faraday's constant (approximately 96485 C/mol).
Step 5: Understand that a negative ΔG indicates a spontaneous reaction, while a positive E indicates a spontaneous reaction in the electrochemical cell.
Step 6: Conclude that if the cell potential (E) is high, the Gibbs free energy (ΔG) will be low (more negative), indicating a favorable reaction.

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