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Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction. Cu2+(aq)+2e−→Cu(s) Part...

Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction. Cu2+(aq)+2e−→Cu(s) Part A How much time would it take for 330 mg of copper to be plated at a current of 6.2 A ? Express your answer using two significant figures. t =

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Answer #1

1st convert the 330 mg to grams.That's 0.330 grams.

multiply that by the molar mass of Cu, which is about 63.546g/mol. You get .00360mol of Cu. now you multiply that by the mol e- ratio for this equation. That is 2 mol of e- per 1 mol of Cu. This leaves you with .007207 mol e-. We then use Faraday's constant, 96500coulombs. We multiply the .007207mol of e- by 96500Coulombs/1mole of e- to give us 695.5119 Coulombs.Then you use the formula Amps*time=Coulombs. You manipulate it to be Time=Coulombs/Amps. So, 695.51C/6.2 Amps=112.1790322 seconds.
Note: time must be in seconds.

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