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A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10. A

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Answer:

This is the answer

Explanation:

charges passed = current x time = 10 x 3 x 60

= 1800 C

mole of charge = 1800 / 96500

= .01865 moles

Au+3 contains 3 positive charges

3 mole of charge will deposit 1 mole of Au .01865 moles will deposit .01865 / 3 mole

= 6.2167 x 10-3 moles.

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