Test 2

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Johnathan Smith 1D
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Joined: Wed Sep 11, 2019 12:16 am

Test 2

Postby Johnathan Smith 1D » Sun Mar 08, 2020 11:05 pm

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?

san_2F
Posts: 118
Joined: Sat Jul 20, 2019 12:15 am

Re: Test 2

Postby san_2F » Sun Mar 08, 2020 11:06 pm

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.

KarineKim2L
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Joined: Fri Aug 30, 2019 12:16 am

Re: Test 2

Postby KarineKim2L » Sun Mar 08, 2020 11:07 pm

The one with the more positive or higher potential will be reduced, and the one with the more negative/smaller potential will be oxidized.

Simon Ketema_1F
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Joined: Wed Nov 13, 2019 12:26 am

Re: Test 2

Postby Simon Ketema_1F » Sun Mar 08, 2020 11:09 pm

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.

Ariel Fern 2B
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Joined: Fri Aug 30, 2019 12:17 am

Re: Test 2

Postby Ariel Fern 2B » Sun Mar 08, 2020 11:10 pm

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!

Althea Zhao 1B
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Joined: Mon Jun 17, 2019 7:24 am

Re: Test 2

Postby Althea Zhao 1B » Sun Mar 08, 2020 11:11 pm

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.

Eugene Chung 3F
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Joined: Wed Nov 15, 2017 3:03 am

Re: Test 2

Postby Eugene Chung 3F » Sun Mar 08, 2020 11:18 pm

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.

Adriana_4F
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Joined: Fri Sep 28, 2018 12:29 am

Re: Test 2

Postby Adriana_4F » Sun Mar 08, 2020 11:20 pm

Since Fe had the lower cell potential it was being oxidized and Ag was being reduced.


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