Moderators: Chem_Mod, Chem_Admin

April P 1C
Posts: 38
Joined: Thu Jan 12, 2017 3:01 am


Postby April P 1C » Thu Feb 22, 2018 3:05 pm

d) Au^(+) (aq) -> Au(s) + Au^(3+) (aq)

Why can't I use
Au+ (aq) -> Au^(3+) (aq)
for the oxidation half reaction?

When I used that I was able to get the correct overall balanced redox reaction. And when I got the cell diagram, couldn't I have placed Pt(s) on the anode side? The solutions don't have this though. Why?

Kaelie Blanes-Ronda 2L
Posts: 42
Joined: Fri Sep 29, 2017 7:07 am
Been upvoted: 1 time

Re: 14.13

Postby Kaelie Blanes-Ronda 2L » Thu Feb 22, 2018 4:21 pm

I'm pretty sure both ways are right especially if you got the right overall balanced reaction. The only way that it would definitely be Au(s) is if the table of reactions shows this reaction of having Au as a solid and aqueous product.

Return to “Balancing Redox Reactions”

Who is online

Users browsing this forum: No registered users and 1 guest