Question

In a particular electroplating process, the metal being plated has a +4 charge. If 861.8 C of charge pass through the cell, how many moles of metal should be plated? Useful information: F = 96,500 C/mol e- Provide your response to four digits after the decimal.

Answer 1

Answer: $2.2326\times 10^{-3}$ moles

Explanation:

We are given:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains $6.022\times 10^{23}$ number of particles.

We know that:

Charge on 1 electron = $1.6\times 10^{-19}C$

Charge on 1 mole of electrons = $1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C$

The metal being plated has a +4 charge, thus the equation will be:

$M^{4+}+4e^-\rightarrow M$

$4\times 96500C$ of electricity deposits = 1 mole of metal

Thus 861.8 C of electricity deposits =$\frac{1}{4\times 96500}\times 861.8=2.2326\times 10^{-3}$ moles of metal

Thus $2.2326\times 10^{-3}$ moles of metal should be plated