In a fuel cell, hydrogen and oxygen react to produce electricity. In process, hydrogen gas is oxidized at the anode and oxygen at the cathode. If `67.2L` of `H_(2)` at `STP` reacts in `15mi n` , what is the average current produced ? If the entire current is used for electro`-` deposition of copper from copper `(II)` solution, how many grams of copper will be deposited ?
Anode reaction `: H_(2)=2overset(c-)(O)Hrarr2H_(2)O+2e^(-)`
Cathode reaction `:O_(2)+2H_(2)O+2e^(-) rarr 4overset(c-)(O)H`

Answer

`190.5g`

Explanation

Moles of `H_(2)` reacting `=(67.2)/(22.4)=3`
`:. `Equivalent of `H_(2)` used `=3xx2=6`
Now, `(W)/(E_(w))=(It)/(96500)`
`:. 6=(Ixx15xx60)/(96500)`
`:.I=643.33A`
Also, equivalent of `H_(2)=` equivalent of `Cu` formed
`:. ` Equivalent of `Cu` deposited `=6`
`:. W_(Cu)=6xx(63.5)/(2)=190.5g`
Thus, weight of `Cu` deposited `=190.5g`