## Electrolysis.

In the electrolysis of Au3+ (aq) solution, gold is deposited. How much gold is deposited in 6 hours by a constant current of 0.540 A?

I know you need to find the moles of e- by using It/F. But I'm not sure where to go from there.

Any help would be great.

Thanks.
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 Blog Entries: 9 Recognitions: Homework Help Science Advisor Use Faraday's law,compute the mass of Au by making those multiplications/divisions and then compare to the fninal result. The formulation's kinda vague,so you can leave the final answer in Kg... Daniel.
 Recognitions: Gold Member Homework Help Consider the half-reaction Au3+(aq) + 3e- -------------> Au(s) Now 1 mol of Au3+ requires 3 Faradays (3*96500 C) to deposit 1 mol of Au Therefore, if the amount of charge passed is 6*3600*.540 C, how many moles of Au will be deposited?

## Electrolysis.

Okie dokie, thanks.
 I just used n = It/zF (where z= amout of "excess" electrons). Then multiplied the answer by the molar mass of gold. That gave me 7.94g.

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