anwser the following question... (please show work so i can follow what you are

Question

anwser the following question... (please show work so i can follow what you are doing)

1.Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equation.) CH2O (l) + Ag+ (aq) + H2O (l) HCO2H (aq) + Ag(s) + H+ (aq)

2. Using the reduction potentials table in the notes/book, which of the following is the best oxidizing agent?

Using the reduction potentials table in the notes/book, which of the following is the best oxidizing agent?

a.MnO4-

F-

Fe2+

I2

a.MnO4-

F-

Fe2+

I2

Explanation / Answer

CH2O (l) + Ag+ (aq) + H2O (l) HCO2H (aq) + Ag(s) + 2 H+ (aq)

Using standard reduction potential table the compound having higher reduction potential than Ag+ would be good oxidizing agent/

F2 + 2e --> 2 F- (aq) { reduction potential 2.87 V}

MnO4- + 8 H3O+ + 5e- --> Mn2+ +12H2O  { reduction potential 1.52 V}

Fe2+ + 2e --> Fe   { reduction potential -0.44 V}

I2 + 2e --> 2 I- { reduction potential 0.54 V}

SInce F2 has higher reduction potential but in option we have F- . So this is incorrect.

Next highest reduction potential value is of MnO4- . Therefore it's a good oxidizing agent.

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