For a hydrogen-oxygen fuel cell at $1 \text{ atm}$ and $298 \text{ K}$, the reaction is $H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_{2}O_{(l)}$; $\Delta G^{\circ} = -240 \text{ kJ}$. The $E^{\circ}$ for the cell is approximately (Given $F = 96,500 \text{ C}$): (in $\text{ V}$)

• A
  $1.24$
• B
  $1.26$
• C
  $2.48$
• D
  $2.5$