The standard reduction potential for the half-reaction:
Sn4+ + 2e- --> Sn2+ is +0.15 V.
For a galvanic cell under standard conditions, which of thefollowing anodic half reactions would produce, at the cathode aspontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn.
Fe --> Fe2+ + 2e-
Pb --> Pb2+ + 2e-
Sn2+ --> Sn4+ + 2e-
Fe --> Fe3+ + 3e-
H2 + 2OH- --> 2H2O + 2e-
Sn --> Sn2+ + 2e-
Sn4+ + 2e- --> Sn2+ is +0.15 V.
For a galvanic cell under standard conditions, which of thefollowing anodic half reactions would produce, at the cathode aspontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn.
Fe --> Fe2+ + 2e-
Pb --> Pb2+ + 2e-
Sn2+ --> Sn4+ + 2e-
Fe --> Fe3+ + 3e-
H2 + 2OH- --> 2H2O + 2e-
Sn --> Sn2+ + 2e-
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Related questions
Standard reduction potentials
| Reduction half-reaction | E∘ (V) |
| Ag+(aq)+e−→Ag(s) | 0.80 |
| Cu2+(aq)+2e−→Cu(s) | 0.34 |
| Sn4+(aq)+4e−→Sn(s) | 0.15 |
| 2H+(aq)+2e−→H2(g) | 0 |
| Ni2+(aq)+2e−→Ni(s) | −0.26 |
| Fe2+(aq)+2e−→Fe(s) | −0.45 |
| Zn2+(aq)+2e−→Zn(s) | −0.76 |
| Al3+(aq)+3e−→Al(s) | −1.66 |
| Mg2+(aq)+2e−→Mg(s) | −2.37 |
Part A
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:
Express your answer numerically.
Part B
Calculate the standard cell potential (E∘) for the reaction
if K = 3.04×10−3.
Express your answer to three significant figures and include the appropriate units.
The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of calomel Hg2Cl2. The electrolyte solution is KCl. ESCE is +0.242 V relative to standard hydrogen electrode.
Calculate the potential for each of the galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in table:
| Electrode |
SCE |
a) Cu2+ + 2e- → Cu | b) Fe3+ + e- → Fe2+ | c) AgCl + e- → Ag + Cl- | d) Al3+ + 3e- → Al | e) Ni2+ + 2e- → Ni |
| Eo |
+0.242 V |
+ 0.339 V | + 0.771 V | + 0.223 V | - 1.677 V | - 0.257 V |
