Need help on these 2 questions: If you can also answer this one, that would be g

Question

Need help on these 2 questions:

If you can also answer this one, that would be great (or at least give me a sketch on paint?):

If a piece of silver is placed in a solution in which [Ag 4] = [Fe 2+] = 1.00 M at STP, what is E cell for the following reaction? Ag(s) + Fe 2+ (aq) rightarrow 2 Ag + (aq) + Fc(s) Rank the following compounds in order of their capacity to act as oxidizing agents. Use the curved arrow tool on the Lewis structures below to show how electron pairs move, and bonds form and break, in this reaction. Note: HSbF 6 is an ionic compound and one of the strongest Br nsted-Lowry acids known.

Explanation / Answer

1)   

Eo cell = EO Fe+2 /Fe - EO Ag+/Ag

Eo cell = -0.44 - 0.80

Eo cell = -1.24 V

E = EO cell - ( 0.0591/n) log Q

here n =2

E= Eo cell - ( 0.0591/2 ) log [Ag+] 2 / [Fe+2]

E = -1.24 - ( 0.0591/2) log 1

E = -1.24

So the value of E is -1.24 V

2) to act as a strong oxidizing agent , the substance should undergo reduction , so the reduction potential should be

highly positive .They should be placed down in the reduction potential table .

SO the order is

Fe+2 < Fe+3 < Hg2 +2 < Hg+2

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