A solution of `CuSO_(4)` is electrolyzed for `10 ` min with a current of `1.5A`. What is the mass of `Cu` deposited at the cathode? `[` Atomic mass of `Cu=63g]`

Explanation

`t=600s` charge=current`xx`time`=1.5Axx600s=900C`
According to the reaction:
`Cu^(2+)(aq)+2e^(-)=Cu(s)`
we require 2F or `2xx96487C` to deposit 1 mol or 63 g of Cu.
. For 900C, the mass of Cu deposited.
`=(63g" "mol^(-1)xx900C)//1(2xx96487C" "mol^(-1))=0.2938g`.