For hydrogen-oxygen fuel cell at 1 atm and 298 K- H 2 g - 1 2 O 2 g - H 2 O l - - G o -240kJ E o for the cell is approximately -Given- F - 96-500 C-

The correct option is B 1.24 V According to the equation: Δ G^o= nFE^o E^o= Δ G^onF=2400002×96500=1.24 V Hence, option A is correct. ...

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Byju's Answer

Standard XII

Chemistry

Fuel Cells

For hydrogen-...

Question

For hydrogen-oxygen fuel cell at $1$ atm and $298 K$ ,

$H_{2 (g)} + \frac{1}{2} O_{2 (g)} ⟶ H_{2} O_{(l)}; Δ G^{o} = - 240 k J$

$E^{o}$ for the cell is approximately :

[Given: $F = 96, 500 C$ ]

1.24 V

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1.26 V

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2.48 V

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2.5 V

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Solution

The correct option is B $1.24 V$
According to the equation:

$Δ G^{o} = - n F E^{o}$

$E^{o} = \frac{- Δ G^{o}}{n F} = \frac{240000}{2 \times 96500} = 1.24 V$

Hence, option A is correct.

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Similar questions

Consider a $70 %$ efficient hydrogen-oxygen fuel cell working under standard conditions at $1 bar$ and $298 K$ . Its cell reaction is

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)$
The work derived from the cell on the consumption of $1.0 \times 10^{- 3} mol$ of $H_{2} (g)$ is used to compress $1.00 mol$ of a monoatomic ideal gas in a thermally insulated container. What is the change in the temperature (in K) of the ideal gas?The standard reduction potentials for the two half-cells are given below.
$O_{2} (g) + 4 H^{+} (a q) + 4 e^{-} \to 2 H_{2} O (l), E^{o} = 1.23 V 2 H^{+} (a q) + 2 e^{-} \to H_{2} (g), E^{o} = 0.00 V$
Use $F = 96500 C m o l^{- 1}, R = 8.314 J m o l^{- 1} K^{- 1}$