Question

The amount of electricity required to produce 12.7 g of
copper from CuSO4 using inert electrode would be
(Atomic mass of Cu = 63.5] (Here F - Faraday).​

Answer 1

First of all, write the half cell reaction:

$Cu^{+2}+2e^{-}\rightarrow Cu$

Now, we can see that :

For 63.5 gram of Cu, we need 2 moles (or 2 F) electricity.

So, for 12.7 gram of Cu , we need :

$= \dfrac{2}{63.5} \times 12.7$

$= 0.4 \: F$

So, 0.4 F of electricity is necessary.

In terms of Coulomb, we can say:

$\implies 0.4 \: F \approx 0.4 \times 96500 = 38600 \: C$

So, 38600 Coulomb of electricity is necessary.