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

Explanation

`C_(6)H_(5)NO_(2)+6H^(+)+6e rarrC_(6)H_(5)NH_(2)+2H_(2)O`
`N^(3+)+6e rarr N^(3-)`
`therefore` Eq. wt. of nitrobenzene `=(M)/(6)=(123)/(6)`
Since current efficiency is 50%
`therefore i=(50i_(0))/(100)`
Now `w=("E.i.t")/(96500), 12.3=(123xxi_(0)xxtxx50)/(6xx100xx96500)`
`therefore i_(0)xx t=115800` coulomb
Now energy used `QxxV=115800xx3=347.4kJ`