What is the relationship between Gibbs free energy and cell potential?
Practice Questions
1 question
Q1
What is the relationship between Gibbs free energy and cell potential?
G = -nFE
G = nFE
G = 0
G = nF/E
The relationship is given by the equation G = -nFE, where G is Gibbs free energy, n is moles of electrons, F is Faraday's constant, and E is cell potential.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the relationship between Gibbs free energy and cell potential?
Solution: The relationship is given by the equation G = -nFE, where G is Gibbs free energy, n is moles of electrons, F is Faraday's constant, and E is cell potential.
Steps: 6
Step 1: Understand that Gibbs free energy (G) 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 a galvanic cell during a redox reaction.
Step 3: Recognize that the equation G = -nFE shows the relationship between Gibbs free energy and cell potential.
Step 4: Identify the variables in the equation: G is Gibbs free energy, n is the number of moles of electrons transferred in the reaction, F is Faraday's constant (approximately 96485 C/mol), and E is the cell potential in volts.
Step 5: Realize that a negative Gibbs free energy (G < 0) indicates a spontaneous reaction, which corresponds to a positive cell potential (E > 0).
Step 6: Conclude that as the cell potential increases, the Gibbs free energy decreases, meaning the reaction becomes more favorable.
