The oxidation of methanol,as described by the equation below,has a $\Delta$G° value of -937.9 kJ/mol.What is the standard cell potential for a methanol fuel cell? 2 CH₃OH( )+ 3 O₂(g)$\to$ 2 CO₂(g)+ 3 H₂O( )

Question

Quizplus · Accepted Answer

The standard cell potential can be calculated using the formula:
ΔG° = -nFE°cell
where:
ΔG° is the standard Gibbs free energy change
n is the number of electrons transferred in the balanced equation
F is the Faraday constant (96,485 C/mol)
E°cell is the standard cell potential

From the balanced equation, we see that n = 11, since 11 electrons are transferred. Therefore:
E°cell = ΔG°/(-nF)
E°cell = (-937.9 kJ/mol)/(-11 × 96,485 C/mol)
E°cell = 0.810 V

Therefore, the correct choice is C, "0.810 V".

The Oxidation of Methanol,as Described by the Equation Below,has A \Delta