Question

10. What is the best reducing agent? Cu+, Ag+, F2, Fe3+
Please explain the step by step of reading the half reaction table, plus the use of signs, whenever it's positive and negative.

11. Sketch the voltaic cell containing Mg/Mg2+ and Pb/Pb2+ half cells. Describe everyrhing that is going on in the cell. Calculate the E°cell.
Please explain the steps.

10. What is the best reducing agent? Cu, Ag'. F2, Fet 11: Sketch the voltaic cell containing Mg/Mg and Pb/Pb2+ half cells. Describe everything that is going on in the cell Calculate the E'cell

Answer 1

If a set of metals have been given then look at most negative value of standard reduction potential will behave as anode and also most reactive metal in the given set. So automatically other metal in the given pair becomes cathode.

Look at Activity series below

most reactive least reactive

Li K Ba Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H2 Cu Hg Ag Pt Au

10) have a look at following

Reduction Half-Reaction	Standard Potential Ered° (V)
F2(g) + 2e– → 2F–(aq)	+2.87
Ag+(aq) + e– → Ag(s)	+0.80
Fe3+(aq) + e– →  Fe2+(aq)	+0.771
Cu+(aq) + e– → Cu(s)	+0.52
Pb2+(aq) + 2e– → Pb(s)	–0.13
Mg2+(aq) + 2e– → Mg(s)	–2.38

Answer: the best reducing agent is least positive one that is Cu⁺

11)

RED Pfleco (current direction) - BLACK Voltmeter (+) Cathode Anode мя - > Pb metal elecbde Metal electrode -> Pb2+ (aq, 1.0M) Mght (aq, 1.0M) V Salt-Bridge (Ntnog in agar-agar gel) E° (Mg) => Mght +2€ Pb2+ + ze = Mgrsi e = -2.38V (Anode) = Pb(s) E= -213V (Cattode) At anode: Mg(s) → might (aq) + 2€ At cathode: Pb2t(aq) + 2€ → Phrs) Net reaction Mg(s) + potlag) -> Mgcaq) + pors) Ecell = Ecatiede -Eanode -0.13 V -(- 2.3) | Ecele = + 2.25 V

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