During the electrolysis of water, a total volume of `33.6mL` of hydrogen and oxygen gas was collected at `STP`. Find the amound of electricity that passed during electrolysis.

Explanation

Cathode `:2H^(o+)+2e^(-) rarr H_(2)`
`implies 2F-=1 mol of H_(2)-=22400mL`
or `1F-=0.5 mol of H_(2)-=11200mL`
Anode`: overset(c-)(O)H rarr O_(2)+4e^(-)+2H_(2)O`
`implies 4F-=1 mol of O_(2)-=22400mL`
or `1F-=0.25 mol of O_(2)-=11200mL`
From two electrode reactions , it is clear that hydrogen and oxygen are evolved in the mole ration of `2:1`, hence their volumes will also be in the same ratio.
`implies ` Volume of `H_(2)=2//3(33.6)=22.4mL`
As `2F-=22400mL H_(2)`
`implies 0.002F` of charge is passed through the electrolytic cell.
`implies` Amount of electricity `=0.002 xx 96500C`
`=193.0C`