## Homework 14.13 D

Ashley Van Belle 2B
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### Homework 14.13 D

The problem asks to write the half-rxns, the balanced equation for the cell reaction, and the cell diagram for Au+(aq) --> Au(s) + Au3+(aq)

How am I supposed to do this problem and determine what would be the cathodes and anodes? With just one reactant, I don't know where to start. The book writes the two half-rxns as 3Au+(aq) + 3e- --> Au(s) for the cathode and Au3+(aq) + 3e- --> Au(s) for the anode. How does this work if for the second half-rxn, both of the products of the equation are the ones involved in the half-rxn?

Chem_Mod
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### Re: Homework 14.13 D

It is seen that when you balance the equation, there will be $Au_{(s)}$ on only one side of the equation. Use the solid Au as the product for both redoxs from +1 Au and +3 Au. When you combine the two, in the form of the reaction given (+1 Au on the left, +3 Au on the right), the form will take place.