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 -237 kJ/mol. What is the standard cell potential for this fuel cell?
H₂(g) + $\frac { 1 } { 2 }$ O₂(g) $\rightarrow$ H₂O(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 -237 kJ/mol. What is the standard cell potential for this fuel cell?
H₂(g) +

\frac { 1 } { 2 }

O₂(g)

\rightarrow

H₂O(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 (2 for this reaction), F is Faraday's constant (96485 C/mol), and $\Delta G°$ is given as -237 kJ/mol. Solving for E° gives approximately 1.23 V.

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