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Standard XII

Chemistry

Faraday's First Law

In a hydrogen...

Question

In a hydrogen-oxygen fuel cell, $67.2 l i t r e$ of $H_{2}$ at STP is used in $15$ minutes. What is the average current produced?

549.4 a m p

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643.33 a m p

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965 a m p

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129.8 a m p

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Solution

The correct option is B $643.33 a m p$
At STP condition we have,
22.4 L of gas require 193000 C

and for for 67.2 L of gas we require = $\frac{193000 \times 67.2}{22.4}$ C
current require = 579000 C

we have, $Q = I t$

$I =$ $\frac{Q}{t}$

$I =$ $\frac{579000}{15 \times 60}$

average current produced = 643.33 amp

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In a hydrogen-oxygen fuel cell, 67.2 litre of H2 at STP is used in 15 minutes. What is the average current produced?

The correct option is B 643.33 ampAt STP condition we have,22.4 L of gas require 193000 Cand for for 67.2 L of gas we require = 193000×67.222.4 Ccurrent require = 579000 Cwe have, Q=ItI= QtI= 57900015×60average current produced = 643.33 amp

In a hydrogen-oxygen fuel cell, $67.2 l i t r e$ of $H_{2}$ at STP is used in $15$ minutes. What is the average current produced?