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( Consider a galvanic cell involving tin(II) and iron (II) and the corresponding Sn and Fe electrodes (use the data in Table 12.1 from the text). Hand draw this galvanic cell include the details below. Select the tickbox when you have completed this question. a) Draw a sketch of the cell b) Clearly identify the anode and cathode c) Write the balanced overall reaction "1

( Consider a galvanic cell involving tin(II) and iron (II) and the corresponding Sn and Fe electrodes (use the data in Table 12.1 from the text). Hand draw this galvanic cell include the details below. Select the tickbox when you have completed this question. a) Draw a sketch of the cell b) Clearly identify the anode and cathode c) Write the balanced overall reaction "1

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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( Consider a galvanic cell involving tin(II) and iron (II) and the corresponding Sn and Fe electrodes (use the data in Table 12.1 from the text). Hand draw this galvanic cell include the details below. Select the tickbox when you have completed this question. a) Draw a sketch of the cell b) Clearly identify the anode and cathode c) Write the balanced overall reaction d) Which electrode will lose mass e) Outline the direction of the electron flow
Transcribed Image Text:( Consider a galvanic cell involving tin(II) and iron (II) and the corresponding Sn and Fe electrodes (use the data in Table 12.1 from the text). Hand draw this galvanic cell include the details below. Select the tickbox when you have completed this question. a) Draw a sketch of the cell b) Clearly identify the anode and cathode c) Write the balanced overall reaction d) Which electrode will lose mass e) Outline the direction of the electron flow
TABLE 12.1 Standard reduction potentials E* at 25 °C Half-reaction Strongest F₂(g) + 2e- oxidising agent (oxidant) S₂O² (aq) + 2e- PbO₂ (s) + HSO4 (aq) + 3H+(aq) + 2e- 2HOCl(aq) + 2H+(aq) + 2e¯ MnO4 (aq) + 8H+ (aq) + 5e- BrO3(aq) + 6H+(aq) + 6e- PbO₂ (s) + 4H+ (aq) + 2e- CIO3(aq) + 6H+(aq) + 6e¯ Au³+ (aq) + 3e- CIO4 (aq) + 8H++ 8e- Cl₂(g) + 2e- O₂(g) + 4H+(aq) + 4e¯ Br₂(aq) + 2e- NO3(aq) + 4H+(aq) + 3e¯ Ag+ (aq) + e- Fe³+ (aq) + e- 1₂(s) + 2e- NiO₂ (s) + 2H₂O(l) + 2e- Cu²+ (aq) + 2e- Cl₂(aq) + 40H-(aq) Hg₂Cl₂(s) + 2e- AgCl(s) + e- SO2-(aq) + 4H+ (aq) + 2e- Sn4+(aq) + 2e- AgBr(s) + e- 2H+(aq) + 2e- Sn²+(aq) + 2e- Ni²+ (aq) + 2e- Co²+ (aq) + 2e- PbSO4(s) + H+(aq) + 2e¯ Cd²+(aq) + 2e- Fe²+ (aq) + 2e- Cr³+ (aq) + 3e- Zn²+ (aq) + 2e- 2H₂O(1) + 2e- Al³+ (aq) + 3e- Mg²+ (aq) + 2e- Na+ (aq) + e- Weakest Ca²+ (aq) + 2e oxidising K+ (aq) + e- agent (oxidant) Lit(aq) + e¯ 12 12 12 12 12 12 12 12 12 2F -(aq) 2SO²-(aq) PbSO4(s) + 2H₂O(1) Cl₂(g) + 2H₂O(1) Mn²+ (aq) + 4H₂O(1) Br-(aq) + 3H₂O(1) Pb²+ (aq) + 2H₂O(1) Cl(aq) + 3H₂O(1) Au(s) CI -(aq) + 4H₂O 2Cl(aq) 2H₂O(1) 2Br (aq) NO(g) + 2H₂O(1) Ag(s) Fe²+ (aq) 21-(aq) Ni(OH)₂(s) + 2OH-(aq) Cu(s) 2OCI-(aq) + 2H₂O(l) + 2e- 2Hg(1) + 2Cl(aq) Ag(s) + CI-(aq) H₂SO3(aq) + H₂O(1) Sn²+ (aq) Ag(s) + Br−(aq) H₂(g) Sn(s) Ni(s) Co(s) Pb(s) + HSO4 (aq) Cd(s) Fe(s) Cr(s) Zn(s) H₂(g) + 2OH-(aq) Al(s) Mg(s) Na(s) Ca(s) K(s) Li(s) E* (volts) +2.87 +2.01 +1.69 +1.63 +1.51 +1.47 +1.46 +1.45 +1.42 +1.38 +1.36 +1.23 +1.07 +0.96 +0.80 +0.77 +0.54 +0.49 +0.34 +0.32 +0.27 +0.23 +0.17 +0.15 +0.07 0 -0.14 -0.25 -0.28 -0.36 -0.40 -0.44 -0.74 -0.76 -0.83 -1.66 -2.37 -2.71 -2.76 -2.92 -3.05 Weakest reducing agent (reductant) Strongest reducing agent (reductant)
Transcribed Image Text:TABLE 12.1 Standard reduction potentials E* at 25 °C Half-reaction Strongest F₂(g) + 2e- oxidising agent (oxidant) S₂O² (aq) + 2e- PbO₂ (s) + HSO4 (aq) + 3H+(aq) + 2e- 2HOCl(aq) + 2H+(aq) + 2e¯ MnO4 (aq) + 8H+ (aq) + 5e- BrO3(aq) + 6H+(aq) + 6e- PbO₂ (s) + 4H+ (aq) + 2e- CIO3(aq) + 6H+(aq) + 6e¯ Au³+ (aq) + 3e- CIO4 (aq) + 8H++ 8e- Cl₂(g) + 2e- O₂(g) + 4H+(aq) + 4e¯ Br₂(aq) + 2e- NO3(aq) + 4H+(aq) + 3e¯ Ag+ (aq) + e- Fe³+ (aq) + e- 1₂(s) + 2e- NiO₂ (s) + 2H₂O(l) + 2e- Cu²+ (aq) + 2e- Cl₂(aq) + 40H-(aq) Hg₂Cl₂(s) + 2e- AgCl(s) + e- SO2-(aq) + 4H+ (aq) + 2e- Sn4+(aq) + 2e- AgBr(s) + e- 2H+(aq) + 2e- Sn²+(aq) + 2e- Ni²+ (aq) + 2e- Co²+ (aq) + 2e- PbSO4(s) + H+(aq) + 2e¯ Cd²+(aq) + 2e- Fe²+ (aq) + 2e- Cr³+ (aq) + 3e- Zn²+ (aq) + 2e- 2H₂O(1) + 2e- Al³+ (aq) + 3e- Mg²+ (aq) + 2e- Na+ (aq) + e- Weakest Ca²+ (aq) + 2e oxidising K+ (aq) + e- agent (oxidant) Lit(aq) + e¯ 12 12 12 12 12 12 12 12 12 2F -(aq) 2SO²-(aq) PbSO4(s) + 2H₂O(1) Cl₂(g) + 2H₂O(1) Mn²+ (aq) + 4H₂O(1) Br-(aq) + 3H₂O(1) Pb²+ (aq) + 2H₂O(1) Cl(aq) + 3H₂O(1) Au(s) CI -(aq) + 4H₂O 2Cl(aq) 2H₂O(1) 2Br (aq) NO(g) + 2H₂O(1) Ag(s) Fe²+ (aq) 21-(aq) Ni(OH)₂(s) + 2OH-(aq) Cu(s) 2OCI-(aq) + 2H₂O(l) + 2e- 2Hg(1) + 2Cl(aq) Ag(s) + CI-(aq) H₂SO3(aq) + H₂O(1) Sn²+ (aq) Ag(s) + Br−(aq) H₂(g) Sn(s) Ni(s) Co(s) Pb(s) + HSO4 (aq) Cd(s) Fe(s) Cr(s) Zn(s) H₂(g) + 2OH-(aq) Al(s) Mg(s) Na(s) Ca(s) K(s) Li(s) E* (volts) +2.87 +2.01 +1.69 +1.63 +1.51 +1.47 +1.46 +1.45 +1.42 +1.38 +1.36 +1.23 +1.07 +0.96 +0.80 +0.77 +0.54 +0.49 +0.34 +0.32 +0.27 +0.23 +0.17 +0.15 +0.07 0 -0.14 -0.25 -0.28 -0.36 -0.40 -0.44 -0.74 -0.76 -0.83 -1.66 -2.37 -2.71 -2.76 -2.92 -3.05 Weakest reducing agent (reductant) Strongest reducing agent (reductant)
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