Calculate the quantity of electricity that would be required to reduce `12.3g` of nitrobenzene to aniline, if the current efficiency for the process is `50%`. If the potential drop across the cell is `3.0V`, how much energy will be consumed?

Answer

`347.4Kj`

Explanation

`C_(6)H_(5)NO_(2)+6H^(o+)+6e^(-) rarr C_(6)H_(5)NH_(2)+2H_(2)O`
`N^(3+)+6e^(-) rarr N^(3-)`
`:. " " `Equivalent weight `(Ew)` of `C_(6)H_(5)NO_(2)=(Mw)/(6)=(123)/(6)`
Now, `W=(Z.I.t)/(96500)`
Since, current efficiency is `50%`
`:. I=(50I_(0))/(100) (I_(0)=` Initial current `)`
`:. 12.3=(123xxIxxtxx50)/(6xx100xx96500)`
`:.I_(0)xxt(i.e.,Q)=115800C`
Now, energy used `=8xxV`
`=115800xx347.4kJ`