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 proc

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))^(-) rarr 4H_(2)O(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 `therefore` no. of moles of hydrogen gas produced `=(1" mole")/(22.4" litres") times 44.8" litres"` = 2 moles of hydrogen `therefore` 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 times 96500C)/(10 times 60s)` I = 643.33 A Electro deposition of copper `Cu^(2+)""_((aq))+2e^(-) rarr 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., 4 F is utilised for electrolysis, then `2 times 63.5` i.e., 127.0 g copper will be deposited at cathode.