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?
2CH₃OH + 3O₂ $\rightarrow$ 2 CO₂ + 3H₂O

Question

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?
2CH₃OH + 3O₂

\rightarrow

2 CO₂ + 3H₂O

Quizplus · Accepted Answer

The standard cell potential can be calculated using the equation:
∆G° = -nFE°cell
where n is the number of electrons transferred in the reaction, F is the Faraday constant (96,485 C/mol), and E°cell is the standard cell potential.

In this case, the oxidation of methanol involves the transfer of 6 electrons, so n = 6. Plugging in the given ∆G° value (-937.9 kJ/mol) and the appropriate constants, we get:

-937.9 kJ/mol = -(6)(96,485 C/mol)(E°cell)
E°cell = 0.810 V

Therefore, the standard cell potential for a methanol fuel cell is 0.810 V.

The Oxidation of Methanol, as Described by the Equation Below Δ\DeltaΔ

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