Final answer:
The value of ΔG° for an electrochemical reaction can be calculated using the formula ΔG° = -nFE°cell, but the number of moles of electrons transferred (n) is required, which is not given in the question.
Step-by-step explanation:
The question asks about the relationship between the standard cell potential (E°cell) and the free energy change (ΔG°) of an electrochemical reaction under standard conditions.
The student wants to determine the ΔG° for a specific reaction using the given E°cell value of 0.500 V.
To calculate the free energy change (ΔG°) for the reaction, we use the formula:
ΔG° = -nFE°cell
where:
n is the number of moles of electrons transferred in the reaction,
F is Faraday's constant (96,485 C/mol e−),
E°cell is the standard cell potential.
However, as the number of moles of electrons (n) isn't provided in the question, we cannot calculate the exact value of ΔG°.
Usually, n corresponds to the balanced overall redox reaction.
Since the half-reactions and stoichiometry are not provided, the student would need this additional information to determine n and proceed with the calculation.