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Homework 14.13 D

Posted: Sun Feb 12, 2017 11:34 pm
by Ashley Van Belle 2B
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?

Re: Homework 14.13 D

Posted: Mon Feb 13, 2017 12:02 am
by Chem_Mod
It is seen that when you balance the equation, there will be 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.