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Question

In a fuel cell, H2 and O2 react to produce electricity. In the process, H2 gas is oxidized at the anode and O2 gas is reduced at the cathode. If 67.2 litres of H2 at STP react in 15 minutes and the entire current is used for electrode deposition of Cu from Cu(II) solution, how many grams of Cu will be deposited and what is the average current produced?
Anode : H2+2OH2H2O+2e
Cathode : O2+2H2O+4e4OH

A
190.5 g of Cu
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B
381 g of Cu
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C
643.33 A
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D
321.6 A
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Solution

The correct option is C 643.33 A
Reaction at anode,
H2(g)2H++2e
67.2 L of H2 ​= 22.42×96500×67.2 coulomb
Time = 15×60 seconds
Average current =2×96500×67.222.4×15×60=643.3 A
Mass of copper deposited by 2×96500×67.222.4 coulomb
=2×96500×63.5×67.22×96500×22.4
=190.5 g.

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