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

To find:

The amount of electricity required to produce 12.7 g of copper from $CuSO_{4}$ using inert electrode.

Calculation:

First, let's write the half cell reaction:

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

Now, from the equation:

• 2F (or 2 moles of electron) is required to get 1 mole (or 63.5 gram) of Copper.

So, amount of electricity needed for 12.7 grams of Copper is:

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

$= 0.4 \: F$

So, amount of electricity needed is 0.4 Faraday (or 0.4 moles of electrons).