Copper is electroplated from CuSO4 solution a constant current of 4 amp is applied by an external power of supply?

How long will it take to deposit 1.00x10^2 g of Cu? The atomic mass of copper is 63.546

1 Answer

  • The reduction half-reaction is Cu2+(aq) + 2 e- --> Cu(s)

    1.00X10^-2 g Cu / 63.546 g/mol = 1.57 mol Cu X 2 mol e- / molCu = 3.15 mol electrons

    3.15 mol e- X 96485 C/mole- = 3.04X10^5 C

    Coulombs = ampere X seconds

    3.04X10^5 C = 4 amp X seconds

    seconds = 7.59X10^4 seconds

    Time = 7.59X10^4 s / 60 = 1265 minutes/60 = 21.1 hours

Hottest videos

Leave a Reply

Your email address will not be published. Required fields are marked *

Related Posts