or the fuel-cell reaction, 2H2 + O2 2H2O, Gº = – 475 kJ. Hence, Eºcell is
Question
or the fuel-cell reaction, 2H2 + O2 2H2O, Gº = – 475 kJ. Hence, Eºcell is
Solution
The standard cell potential (Eºcell) can be calculated from the standard Gibbs free energy change (ΔGº) using the following formula:
ΔGº = -nFEºcell
Where: ΔGº = standard Gibbs free energy change n = number of moles of electrons transferred in the balanced chemical equation F = Faraday's constant (approximately 96485 C/mol) Eºcell = standard cell potential
In the given reaction, 2H2 + O2 → 2H2O, 4 moles of electrons are transferred (2 moles of H2 each gives 2 electrons).
So, we can rearrange the formula to solve for Eºcell:
Eºcell = -ΔGº / (nF)
Substituting the given values:
Eºcell = -(-475,000 J) / (4 * 96485 C/mol)
Eºcell = 1.23 volts
So, the standard cell potential for the given reaction is 1.23 volts.
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