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following questions: Draw the hypothetical galvanic cell Formulate and balance the half-reactions at the anode and cathode. Calculate the standard cell potential (or voltage) generated during the redox reactions at the anode and cathode; Include the cell diagram/notation

following questions: Draw the hypothetical galvanic cell Formulate and balance the half-reactions at the anode and cathode. Calculate the standard cell potential (or voltage) generated during the redox reactions at the anode and cathode; Include the cell diagram/notation

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 33QRT: Consider these half-reactions: (a) Which is the weakest oxidizing agent? (b) Which is the strongest...
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Direction: Choose two (2) elements for the galvanic cell in the table below. Afterward, do and answer the following questions:

  • Draw the hypothetical galvanic cell
  • Formulate and balance the half-reactions at the anode and cathode.
  • Calculate the standard cell potential (or voltage) generated during the redox reactions at the anode and cathode; Include the cell diagram/notation
  • Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness. 
Reduction Half-Reactions Au³+ (aq) + 3e- → Au (s) Ag+ (aq) + e- → Ag (s) Hg₂2+ (aq) + 2e → 2Hg (1) Cu²+ (aq) + 2e → Cu (s) Sn4+ (aq) + 2e- Ni2+ (aq) + 2e →→ Ni (s) Co2+ (aq) + 2e →→ Co (s) Fe (s) Fe2+ (aq) + 2e → Cr³+ (aq) + 3e → Cr (s) Zn²+ (aq) + 2e → Zn (s) Mn²+ (aq) + 2e → Mn (s) Al³+ (aq) + 3e → Al (s) Be2+ (aq) + 2e →→ Be (s) Mg2+ (aq) + 2e → Mg (s) Sn²+ (aq) Na+ (aq) + e- → Na (s) Ca2+ (aq) + 2e → Ca (s) Sr²+ (aq) + 2e →→ Sr (s) Ba2+ (aq) + 2e →→ Ba (s) → K (s) → Li (s) K+ (aq) + e- Li+ (aq) + e- Ered, V 1.520 0.799 0.796 0.340 0.154 -0.257 -0.277 -0.440 -0.744 -0.763 -1.182 -1.676 -1.850 -2.357 -2.714 -2.840 -2.890 -2.920 -2.930 -3.050
Transcribed Image Text:Reduction Half-Reactions Au³+ (aq) + 3e- → Au (s) Ag+ (aq) + e- → Ag (s) Hg₂2+ (aq) + 2e → 2Hg (1) Cu²+ (aq) + 2e → Cu (s) Sn4+ (aq) + 2e- Ni2+ (aq) + 2e →→ Ni (s) Co2+ (aq) + 2e →→ Co (s) Fe (s) Fe2+ (aq) + 2e → Cr³+ (aq) + 3e → Cr (s) Zn²+ (aq) + 2e → Zn (s) Mn²+ (aq) + 2e → Mn (s) Al³+ (aq) + 3e → Al (s) Be2+ (aq) + 2e →→ Be (s) Mg2+ (aq) + 2e → Mg (s) Sn²+ (aq) Na+ (aq) + e- → Na (s) Ca2+ (aq) + 2e → Ca (s) Sr²+ (aq) + 2e →→ Sr (s) Ba2+ (aq) + 2e →→ Ba (s) → K (s) → Li (s) K+ (aq) + e- Li+ (aq) + e- Ered, V 1.520 0.799 0.796 0.340 0.154 -0.257 -0.277 -0.440 -0.744 -0.763 -1.182 -1.676 -1.850 -2.357 -2.714 -2.840 -2.890 -2.920 -2.930 -3.050
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Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness.  

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