In fuel cell H_2 and O_2 react to produce electricity . In the process, H_2 gas is oxidised at the anode and O_2 at cathode. If 44.8 litre of H_2 at 25^@C and also pressure reacts in 10 minutes, what is average current produced ? If the entire current is used for electro deposition of Cu from Cu^(2+) , how many grams of Cu deposited ?

In fuel cell H_2 and O_2 react to produce electricity . In the process

1.	In fuel cell H_2 and O_2 react to produce electricity . In the process, H_2 gas is oxidised at the anode and O_2 at cathode. If 44.8 litre of H_2 at 25^@C and also pressure reacts in 10 minutes, what is average current produced ? If the entire current is used for electro deposition of Cu from Cu^(2+) , how many grams of Cu deposited ?
Answer» Solution :Oxidation at anode : `2H_2(g) + 4OH^(-)(aq) to 4H_2O(l) + 4e^(-)` 1 mole of hydrogen gas produces 2 moles of electrons at `25^@C` and 1 atm pressure, 1 mole of hydrogen gas occupies = 22.4 litres. `:.` no. of moles of hydrogen gas produced = `(1"mole")/(22.4 "litres") xx 44.8` litres = 2 moles of hydrogen `:.` 2 of moles of hydrogen produces 4 moles of ELECTRO i.e., 4F CHARGE. We know that `Q = It` `I = Q/t = (4F)/(10 "mins") = (4 xx 96500 C)/(10 xx 60S)` `I = 643.33 A` Electro deposition of COPPER `Cu_((aq))^(2+) + 2e^(-) to Cu(s)` 2F charge is REQUIRED to deposit 1 mole of copper i.e., 63.5 g If the entire current produced in the fuel cell i.e., 4F is utilised for electrolysis, then `2 xx 63.5` i.e, 127.0 g copper will be deposited at cathode.