electricity. In the process `H_(2)` gas is oxidized at the anode and `O_(2)` at cathode. If `67.2` litre of `H_(2)` st S.T.P reacts in 15 minute, what is average current produced ? If the entire current is used for electro-deposition of Cu from `Cu^(2+)`, how many gram of Cu are deposite ?
Cathode : `O_(2)+2H_(2)O+4e^(-)rarr4OH^(-)`
Anode : `H_(2)+2OH^(-)rarr 2H_(2)+2e^(-)`

Explanation

We know,
Mole of `H_(2)` reacting `=(67.2)/(22.4)=3`
`therefore` Eq. of `H_(2)` used `=3xx2=6`
Now `(w)/(E )=(i.t)/(96500), 6=(ixx15xx60)/(96500)`
`therefore i=643.33` ampere
Also Eq. of `h_(2)` = Eq. of Cu formed
`therefore` Eq. of Cu deposited = 6
`therefore w_(Cu)=6xx(63.5)/(2)=190.5g`
Wt. of Cu deposited `= 190.5g`