Test 2
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Test 2
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
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.
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Re: Test 2
The one with the more positive or higher potential will be reduced, and the one with the more negative/smaller potential will be oxidized.
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Re: Test 2
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.
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Re: Test 2
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!
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Re: Test 2
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.
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Re: Test 2
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.
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