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4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which was reduced. Show all of your work. Redox reaction: Cu(s) +2 Fe³* (aq) → Cu²* (aq) + 2 Fe²* (aq)

4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which was reduced. Show all of your work. Redox reaction: Cu(s) +2 Fe³* (aq) → Cu²* (aq) + 2 Fe²* (aq)

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.101QE: At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction...
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4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which was reduced. Show all of your work. Redox reaction: Cu(s) + 2 Fe" (aq) → Cu?+ (aq) + 2 Fe?+ (aq) Table 1. Standard reduction potentials. Half-Reaction E°(Volts) F,(g) + 2e → 2F(aq) CI, (g) + 2e → 2CI(aq) +2.87 +1.36 Br, () + 2e → 2Br(aq) +1.07 Ag*(aq) + e¯ → Ag(s) +0.80 Fe3*(aq) + e' → Fe2*(aq) +0.77 Cu²"(aq) + 2e' → Cu(s) +0.34 2H*(aq) + 2e¨ → H,(g) 0.00 Fe2*(aq) + 2e' → Fe(s) -0.44 Zn"(aq) + 2e' → Zn(s) -0.76 Al³*(aq) + 3e' → Al(s) -1.66 Mg2 (aq) + 2e → Mg(s) -2.37 Caа" (аg) + 2е > Ca(s) -2.87 K*(aq) + e' → K(s) -2.93 B O Word(s)
Transcribed Image Text:4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which was reduced. Show all of your work. Redox reaction: Cu(s) + 2 Fe" (aq) → Cu?+ (aq) + 2 Fe?+ (aq) Table 1. Standard reduction potentials. Half-Reaction E°(Volts) F,(g) + 2e → 2F(aq) CI, (g) + 2e → 2CI(aq) +2.87 +1.36 Br, () + 2e → 2Br(aq) +1.07 Ag*(aq) + e¯ → Ag(s) +0.80 Fe3*(aq) + e' → Fe2*(aq) +0.77 Cu²"(aq) + 2e' → Cu(s) +0.34 2H*(aq) + 2e¨ → H,(g) 0.00 Fe2*(aq) + 2e' → Fe(s) -0.44 Zn"(aq) + 2e' → Zn(s) -0.76 Al³*(aq) + 3e' → Al(s) -1.66 Mg2 (aq) + 2e → Mg(s) -2.37 Caа" (аg) + 2е > Ca(s) -2.87 K*(aq) + e' → K(s) -2.93 B O Word(s)
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