Silver can exist in two oxidation states, the more common silver(I) and the rare

Question

Silver can exist in two oxidation states, the more common silver(I) and the rarer silver (II):

Ag+ (aq) + e- Ag (s) E o = +0.80 V

Ag2+ (aq) + e- Ag+ (aq) E o = +1.98 V

i. Is the silver (I) ion a good oxidizing agent or a good reducing agent?

ii. Which of the following is the most feasible reagent for oxidizing silver(I) to silver (II): difluorine, fluoride ion, diiodine or iodide ion?

iii. You are thinking of preparing silver (I) hydride, for which: 1/2H2(g) + e- H- (aq) E o = -2.25V

Do you think the compound is likely to be thermodynamically stable? Explain your reasoning.

and

Explain why water with high concentrations of dissolved carbon dioxide and open to atmospheric oxygen is very corrosion towards iron. Consult an appropriate Pourbaix diagram in formulating your answer.

Explanation / Answer

i

Silve will be very good reducing itself, so it must "take" electronsr eadily, therefore a good oxidant

ii

We need a very oxidant material...

Difluorine is the most oxidizing material from the lsit

iii

Not likely, since the E° value is pretty low, also H- is not likely to remain as elemental H

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.