The oxidation of hydrogen by oxygen is one of the most-used reactions in fuel-cell technology. The overall reaction, which is given below, has a $\Delta$ G° value of -474 kJ/mol. What is the standard cell potential for this fuel cell?
2H₂(g) + O₂(g) $\rightarrow$ 2H₂O(l)

Question

The oxidation of hydrogen by oxygen is one of the most-used reactions in fuel-cell technology. The overall reaction, which is given below, has a

\Delta

G° value of -474 kJ/mol. What is the standard cell potential for this fuel cell?
2H₂(g) + O₂(g)

\rightarrow

2H₂O(l)

Quizplus · Accepted Answer

The standard cell potential ($E°$) can be calculated using the formula $\Delta G° = -nFE°$, where $n$ is the number of moles of electrons transferred (4 for this reaction), $F$ is Faraday's constant (96485 C/mol), and $\Delta G°$ is given as -474 kJ/mol. Solving for $E°$ gives approximately 1.23 V.

The Oxidation of Hydrogen by Oxygen Is One of the Most-Used