Determine the molar mass of copper and Faraday's constant.

• Molar mass of copper ($M_{Cu}$) = $63.5 \text{ g/mol}$
• Faraday's constant ($F$) = $96485 \text{ C/mol e⁻}$

Assuming copper is in the +2 oxidation state, the reduction half-reaction is:

This reaction shows that 2 moles of electrons are required to liberate 1 mole of copper.

Given mass of copper ($m$) = $10 \text{ g}$.
Number of moles ($n_{Cu}$) = $\frac{\text{mass}}{\text{molar mass}}$

From the half-reaction, 2 moles of electrons are needed per mole of copper.
Moles of electrons ($n_e$) = $n_{Cu} \times 2$

Quantity of electricity ($Q$) = $n_e \times F$

Rounding to three significant figures:

The quantity of electricity required is: