What is ΔrG° (in kJ mol-1) for a redox reaction that has E°cell = -2.69 V at 25°C ? Assume 4 electrons are transferred in the balanced redox reaction.If needed, F = 96485 C/mol.Answer:Question 4
Question
What is ΔrG° (in kJ mol-1) for a redox reaction that has E°cell = -2.69 V at 25°C ? Assume 4 electrons are transferred in the balanced redox reaction.If needed, F = 96485 C/mol.Answer:Question 4
Solution
To calculate the standard Gibbs free energy change (ΔrG°) for a redox reaction, we can use the following equation:
ΔrG° = -nFE°cell
where: n = number of moles of electrons transferred in the redox reaction F = Faraday's constant (96485 C/mol) E°cell = standard cell potential
Given in the problem, we have: n = 4 F = 96485 C/mol E°cell = -2.69 V
Substituting these values into the equation, we get:
ΔrG° = -4 * 96485 C/mol * -2.69 V
Solving this, we get:
ΔrG° = 1037956.6 J/mol
Since the standard unit for Gibbs free energy change is kJ/mol, we need to convert J/mol to kJ/mol by dividing by 1000:
ΔrG° = 1037956.6 J/mol / 1000 = 1037.9566 kJ/mol
So, the standard Gibbs free energy change (ΔrG°) for the given redox reaction is approximately 1038 kJ/mol.
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