Hi, I had a few questions within the 6M Exercises section (see attachments).
Question 5 part a: Why do we not have to include water in the galvanic cell diagram? And how do we construct the galvanic cell from the given reaction?
Question 7: For this question, do we analyze the stronger reducing agent by looking at standard reduction potentials only? Or are there trends we can observe such as through the periodic table?
Question 11a: What does the Co^2+/Co and Ti^3+/Ti mean?
Is it just reactant/product: e.g. [2e- +Co^2+---> Co ? ]
Question 11d: How do we tell where the "OH-", "O3" and "O2" go in the galvanic cell diagram? Are they at the cathode because they have the higher reduction potential?
6M Exercises (5, 7, 11) [ENDORSED]
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Re: 6M Exercises (5, 7, 11)
5a: Since water is in such large excess, its concentration more or less doesn't change, and it doesn't need to be accounted for in calculations of the galvanic cell.
7: Generally reduction potentials are corelated to electronegativity, so the alkali metals will have low reduction potentials, and the potential will increase going across the periodic table, but you really need to look and the reduction potential table to definitively determine the strength of a reducing agent.
11a: Co^2+/Co and Ti^3+/Ti is a shorthand for the reduction potential equation, similar to the ones you will see in the reduction potential table.
11d: the "OH-", "O3" and "O2" are all part of the same reduction equation, so they will all be on the same side of the galvanic cell diagram, but they are the one being reduced (oxidizing agent) and subsequently on the cathode side because they have a higher reduction potential.
7: Generally reduction potentials are corelated to electronegativity, so the alkali metals will have low reduction potentials, and the potential will increase going across the periodic table, but you really need to look and the reduction potential table to definitively determine the strength of a reducing agent.
11a: Co^2+/Co and Ti^3+/Ti is a shorthand for the reduction potential equation, similar to the ones you will see in the reduction potential table.
11d: the "OH-", "O3" and "O2" are all part of the same reduction equation, so they will all be on the same side of the galvanic cell diagram, but they are the one being reduced (oxidizing agent) and subsequently on the cathode side because they have a higher reduction potential.
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Re: 6M Exercises (5, 7, 11) [ENDORSED]
Great answers.
Whenever (aq) is given it means water is present and therefore no need to explicitly state H2O.
When (aq) is stated then that means water is present and can be part of the redox reaction.
The oxygen atom in water is 2- oxidation state.
The oxygen atom in O2(g) is zero oxidation state.
See the list of standard reduction potentials showing the balanced half reactions involving water.
Whenever (aq) is given it means water is present and therefore no need to explicitly state H2O.
When (aq) is stated then that means water is present and can be part of the redox reaction.
The oxygen atom in water is 2- oxidation state.
The oxygen atom in O2(g) is zero oxidation state.
See the list of standard reduction potentials showing the balanced half reactions involving water.
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