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Problem 4. (25 pts) One-half cell consists of a pure Sn (tin) in a solution of Sn$^{2+}$ ions, the other half cell is a magnesium electrode immersed in a Mg$^{2+}$ solution. Reaction Standard Atomic Atomic Weight Density Potential (V) Number (amu) (g/cm$^3$) Sn$^{2+}$ + 2e$^-$ $\rightarrow$ Sn -0.136 50 118.71 7.27 Mg$^{2+}$ + 2e$^-$ $\rightarrow$ Mg -2.363 12 24.31 1.72 (a) (5 pts) Under standard conditions, write the spontaneous overall reaction and calculate the voltage generated. Describe which electrodes are cathode/anode. (b) (5 pts) Compute the cell potential at 25 $^\circ$C in the Sn$^{2+}$ and Mg$^{2+}$ concentrations are 0.2 and 10$^{-2}$ M, respectively. Calculate the voltage generated, and write the spontaneous overall reaction. Describe the redox process. (c) (10 pts) For (b), if a current of 1 $\mu$A (constant) flows for 1 day, calculate how much material we have gained and lost for both electrodes. (Faraday's constant F=96500 C/mol) Assume no voltage drop during current flow. (d) (5 pts) According to the results in (b) and (c), how would you protect the materials from corrosion? Describe all the options available.

          Problem 4. (25 pts) One-half cell consists of a pure Sn (tin) in a solution of Sn$^{2+}$ ions, the other half cell is a magnesium electrode immersed in a Mg$^{2+}$ solution.

Reaction
Standard
Atomic
Atomic Weight
Density
Potential (V)
Number
(amu)
(g/cm$^3$)
Sn$^{2+}$ + 2e$^-$ $\rightarrow$ Sn
-0.136
50
118.71
7.27
Mg$^{2+}$ + 2e$^-$ $\rightarrow$ Mg
-2.363
12
24.31
1.72
(a) (5 pts) Under standard conditions, write the spontaneous overall reaction and calculate the voltage generated. Describe which electrodes are cathode/anode.
(b) (5 pts) Compute the cell potential at 25 $^\circ$C in the Sn$^{2+}$ and Mg$^{2+}$ concentrations are 0.2 and 10$^{-2}$ M, respectively. Calculate the voltage generated, and write the spontaneous overall reaction. Describe the redox process.
(c) (10 pts) For (b), if a current of 1 $\mu$A (constant) flows for 1 day, calculate how much material we have gained and lost for both electrodes. (Faraday's constant F=96500 C/mol) Assume no voltage drop during current flow.
(d) (5 pts) According to the results in (b) and (c), how would you protect the materials from corrosion? Describe all the options available.

Problem 4. (25 pts) One-half cell consists of a pure Sn (tin) in a solution of Sn^2+ ions, the other half cell is a magnesium electrode immersed in a Mg^2+ solution.

Reaction
Standard
Atomic
Atomic Weight
Density
Potential (V)
Number
(amu)
(g/cm^3)
Sn^2+ + 2e^- → Sn
-0.136
50
118.71
7.27
Mg^2+ + 2e^- → Mg
-2.363
12
24.31
1.72
(a) (5 pts) Under standard conditions, write the spontaneous overall reaction and calculate the voltage generated. Describe which electrodes are cathode/anode.
(b) (5 pts) Compute the cell potential at 25 ^∘C in the Sn^2+ and Mg^2+ concentrations are 0.2 and 10^-2 M, respectively. Calculate the voltage generated, and write the spontaneous overall reaction. Describe the redox process.
(c) (10 pts) For (b), if a current of 1 μA (constant) flows for 1 day, calculate how much material we have gained and lost for both electrodes. (Faraday's constant F=96500 C/mol) Assume no voltage drop during current flow.
(d) (5 pts) According to the results in (b) and (c), how would you protect the materials from corrosion? Describe all the options available.

Added by Julie W.

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