Multiple Choice
What is the equilibrium constant (K) at 305 K when the standard Gibbs free energy change (ΔG°) is +1.61 kJ/mol?
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19. Chemical Thermodynamics
Gibbs Free Energy Calculations
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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 = -0.206 V?
A
-39.8 kJ/mol
B
-19.9 kJ/mol
C
39.8 kJ/mol
D
19.9 kJ/mol
Verified step by step guidance1
Understand the relationship between Gibbs free energy change (ΔG°) and the standard cell potential (E°cell) using the formula: 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.
Identify the number of electrons transferred in the reaction, which is given as 2 electrons. This means n = 2.
Recognize that the standard cell potential (E°cell) is provided as -0.206 V. This value will be used in the formula to calculate ΔG°.
Substitute the known values into the formula: ΔG° = -nFE°cell. Use n = 2, F = 96485 C/mol, and E°cell = -0.206 V.
Perform the calculation by multiplying the values: ΔG° = -(2)(96485 C/mol)(-0.206 V). Remember to convert the result from joules to kilojoules by dividing by 1000, since 1 kJ = 1000 J.
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