Question

What mass of Cu(s) is electroplated by running 19.5 A of current through a Cu2 (aq) solution for 4.00 h

Answer 1

92.46 g

Step-by-step explanation:

The reaction is

`Cu^(2+)+2e^-\rightarrow Cu`

I = Current = 19.5 A

t = 4 hours =
`4* 60* 60=14400\ \text{s}`

F = Faraday constant = 96485.33 C/mol

Molar mass of copper = 63.546 g/mol

Charge is given by

`Q=It\\\Rightarrow Q=19.5* 14400\\\Rightarrow Q=280800\ \text{C}`

Moles of electrons is given by

`(Q)/(F)=(280800)/(96485.33)\\ =2.91\ \text{mol}`

Moles of copper is

`(1)/(2)* (Q)/(F)=(1)/(2)* 2.91\\ =1.455\ \text{mol}`

Mass of copper would be

`\text{Moles}* \text{Molar mass of copper}=1.455* 63.546\\ =92.46\ \text{g}`

The mass of copper electroplated is 92.46 g.