Test 2 #6

Moderators: Chem_Mod, Chem_Admin

Natalie LeRaybaud 1G
Posts: 54
Joined: Thu Jul 13, 2017 3:00 am

Test 2 #6

Postby Natalie LeRaybaud 1G » Thu Mar 15, 2018 2:10 pm

How can you tell what is being oxidized and reduced in this equation? And what is the cell diagram supposed to look like?
The problem is:

The following redox couple forms a galvanic cell which generates a current under standard conditions. O3/O2, OH- and O3,H+/O2

Ishan Saha 1L
Posts: 60
Joined: Fri Sep 29, 2017 7:03 am

Re: Test 2 #6

Postby Ishan Saha 1L » Thu Mar 15, 2018 2:39 pm

We were supposed to use the half reactions on the back sheet provided to us. By comparing the two reactions, we can find which reaction will take place in the anode by looking at the one with the lower reduction potential. This means that this should be an oxidation reaction, so we can flip the equation. We can then look at the change in charges between the oxygen on each side of both reactions to figure out that O3 is the oxidizing agent (since it is being reduced) and 02 is the reducing agent (since it is being oxidized).

Ishan Saha 1L
Posts: 60
Joined: Fri Sep 29, 2017 7:03 am

Re: Test 2 #6

Postby Ishan Saha 1L » Thu Mar 15, 2018 2:41 pm

The Cell Diagram should be Pt(s)|O3(g),O2(g)|OH-(aq)||O2(g),O3(g)|H+(aq)|Pt(s)

Justin Folk 3I
Posts: 43
Joined: Wed Sep 21, 2016 2:56 pm

Re: Test 2 #6

Postby Justin Folk 3I » Thu Mar 15, 2018 6:38 pm

You can tell because of the cell potentials. Overall cell potential has to be positive.


Return to “Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams”

Who is online

Users browsing this forum: No registered users and 1 guest