Multiple Choice
In an electrochemical cell, if the Gibbs free energy change (ΔG) is positive, what can be said about the cell potential (E°cell)?
391
views
20. Electrochemistry
Cell Potential and Gibbs Free Energy
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is ΔG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°_cell = -0.273 V?
A
-52.6 kJ/mol
B
-26.3 kJ/mol
C
26.3 kJ/mol
D
52.6 kJ/mol
Verified step by step guidance1
Identify the formula to calculate the standard Gibbs free energy change (ΔG°) for a redox reaction: ΔG° = -nFE°_cell, where n is the number of moles of electrons transferred, F is the Faraday constant (approximately 96485 C/mol), and E°_cell is the standard cell potential.
Determine the number of moles of electrons transferred in the reaction. In this problem, n = 2 electrons.
Substitute the given values into the formula: n = 2, F = 96485 C/mol, and E°_cell = -0.273 V.
Calculate the product of n, F, and E°_cell. Remember that the units of F (C/mol) and E°_cell (V) will result in the energy being in joules per mole (J/mol).
Convert the energy from joules per mole to kilojoules per mole (kJ/mol) by dividing the result by 1000.
1:28mWatch next
Master Cell Potential and Gibbs Free Energy with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Cell Potential and Gibbs Free Energy practice set
Problem sets built by lead tutorsExpert video explanations