A fuel cell uses $C H_{4} (g) a n d$ forms $C O_{3}^{2 -}$ at the anode. It is used to power a car with 80 Amp for 1 hour. How many liters of $C H_{4} (g)$ (at STP) would be required? $(V_{m} = 22.7 L / m o l & F = 96500 C o u l u m b s)$ . Assume 100% efficiency.

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8.05 L

8.47 L

4.18 L

4.04 L

answer is B.

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Detailed Solution

$C H_{4} + 10 O H^{-} \to_{}^{} C O_{3}^{2 -} + 7 H_{2} O + 8 e^{-}$

$N o . o f F a r a d a y s r e q u i r e d = \frac{1}{8} \times \frac{80 \times 3600 \times 1}{96500}$

$V_{C H_{4}} = \frac{1}{8} \times \frac{80 \times 3600 \times 1}{96500} \times 22.7 L = 8.47 L$

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