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Test 2

Posted: Sun Mar 08, 2020 11:05 pm
by Johnathan Smith 1D
On test two we were given two half reactions and their potentials. How do we know which one is the redox half reaction and which one is the oxidation half reaction?

Re: Test 2

Posted: Sun Mar 08, 2020 11:06 pm
by san_2F
The one with the lower cell potential represents the oxidation half reaction and the one with the higher cell potential represents the reduction half reaction.

Re: Test 2

Posted: Sun Mar 08, 2020 11:07 pm
by KarineKim2L
The one with the more positive or higher potential will be reduced, and the one with the more negative/smaller potential will be oxidized.

Re: Test 2

Posted: Sun Mar 08, 2020 11:09 pm
by Simon Ketema_1F
The more positive half reaction gets reduced, while the more negative half reaction is oxidized. The way I remember it is that the number represents how much a reaction is inclined to be reduced, and the one with the larger value ends up getting reduced.

Re: Test 2

Posted: Sun Mar 08, 2020 11:10 pm
by Ariel Fern 2B
Since it is a Galvanic cell, the E°Cell had to be positive; thus, based on the equation E°Cell = E°Cathode (Reduction) - E°Anode (Oxidation), the Reduction Half Rxn. was the half Rxn. with the more positive E°, and the Oxidation Half Rxn. was the one with the least (most negative) E°. Hope this helps!

Re: Test 2

Posted: Sun Mar 08, 2020 11:11 pm
by Althea Zhao 1B
Since E(cell) is equal to E(red)-E(ox) and must be positive for a spontaneous reaction, E(red) should be greater than E(ox). So, the half reaction with the greater reduction potential is reduced.

Re: Test 2

Posted: Sun Mar 08, 2020 11:18 pm
by Eugene Chung 3F
We know that lower electronegativity and more negative E value means stronger reducing agent. Anode is oxidized and is the reducing agent. So, the one with more negative E value is conventionally the anode.

Re: Test 2

Posted: Sun Mar 08, 2020 11:20 pm
by Adriana_4F
Since Fe had the lower cell potential it was being oxidized and Ag was being reduced.