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

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

How much time would it take for 321mg of copper to be plated at a current of 7.1A ?

Express your answer using two significant figures.

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Homework Answers

Answer #1

We know that

Where W = mass of metal deposited = 321 mg = 321x10-3 g

           E = Equivalent weight of Cu = 63.54 / 2 = 31.77

           C = current = 7.1 A

           t = time taken = ?

Plug the values we get

                                 

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