Answer:
92.46 g
Explanation:
The reaction is
[tex]Cu^{2+}+2e^-\rightarrow Cu[/tex]
I = Current = 19.5 A
t = 4 hours = [tex]4\times 60\times 60=14400\ \text{s}[/tex]
F = Faraday constant = 96485.33 C/mol
Molar mass of copper = 63.546 g/mol
Charge is given by
[tex]Q=It\\\Rightarrow Q=19.5\times 14400\\\Rightarrow Q=280800\ \text{C}[/tex]
Moles of electrons is given by
[tex]\dfrac{Q}{F}=\dfrac{280800}{96485.33}\\ =2.91\ \text{mol}[/tex]
Moles of copper is
[tex]\dfrac{1}{2}\times \dfrac{Q}{F}=\dfrac{1}{2}\times 2.91\\ =1.455\ \text{mol}[/tex]
Mass of copper would be
[tex]\text{Moles}\times \text{Molar mass of copper}=1.455\times 63.546\\ =92.46\ \text{g}[/tex]
The mass of copper electroplated is 92.46 g.
