A current of 3.53 A is passed through a Cu ( NO 3 ) 2 solution for 1.20 h . How much copper is plated out of the solution?

10.035 g of Cu deposited.

Explanation:

Equation of the reaction:

Cu(NO3)2 --> Cu2+ + 2NO3^-

Q = It

Where,

I = current

= 3.53 A

t = time

= 1.2 h * 3600 s/1 h

= 4320 s

Q = 4320 * 3.52

= 15249.6 C

1 mole of metal deposited contains 96500C.

Therefore,

Number of moles = 15249.6/96500

= 0.158 mol of Cu deposited.

Mass = number of moles * molar mass

= 0.158 * 63.5

= 10.035 g of Cu deposited.