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Given the cell notation: Fe/Fe²+ (0.100M)//Cd²+ (0.001)/Cd Write the cell reaction a. b. Calculate Ecell, give polarity of the electrodes and direction of the spontaneous reaction. Calculate Keq. C.

Given the cell notation: Fe/Fe²+ (0.100M)//Cd²+ (0.001)/Cd Write the cell reaction a. b. Calculate Ecell, give polarity of the electrodes and direction of the spontaneous reaction. Calculate Keq. C.

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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Answer the following questions. Refer to the tables for values of Eo. Please show complete solutions.

Given the cell notation: Fe/Fe²+ Write the cell reaction b. Calculate Ecell, give polarity of the electrodes and direction of the spontaneous reaction. Calculate Keq. ܩ C. (0.100M)//Cd²+(0.001)/Cd
Transcribed Image Text:Given the cell notation: Fe/Fe²+ Write the cell reaction b. Calculate Ecell, give polarity of the electrodes and direction of the spontaneous reaction. Calculate Keq. ܩ C. (0.100M)//Cd²+(0.001)/Cd
TABLE 21-2 Element Li K Ca Na Mg Al Zn Cr Fe 2 3 2 5 2 3 2 2 3 2 Cd Ni Sn Pb 1₂ Hg Ag Br₂ Cl₂ Au F₂ TABLE 21-3 reduction of Increasing strength as oxidizing agent; ease increasing Just Buraptxo se Buons Butstanbu Standard Aqueous Reduction Potentials in Aqueous Solution at 25°C Standard Reduction Potential E (volts) increasing ease of reduction Reduction Half-Reaction Lit + e K+ + e¯ Ca²+ + 2e¯ Na+ + e- 2+ Mg²+ + 2e Al³+ + 3e¯ Zn²+ + 2e- Cr³+ + 3e¯ Fe²+ + 2e¯ Cd²+ + 2e- Ni²+ + 2e Sn²+ + 2e¯ Pb²+ 2e 2H+ + 2e™ Cu²+ + 2e¯ Zn(OH)4² +2e™ Fe(OH)₂ + 2e™ 2H₂O + 2e¯ PbSO4 + 2e¯ NO₂ + H₂O + 2e¯ 4+ Sn++ + 2e¯ AgCl + e Hg₂Cl₂ + 2e O₂ + 2H₂O + 4e¯ NiO₂ + 2H₂O + 2e¯ H₂AsO4 + 2H+ + 2e¯ 111 Fe³+ + e CIO + H₂O + 2e¯ NO₂ + 4H+ + 3e¯ O₂ + 4H+ + 4e¯ Cr₂O7²- + 14H+ + 6e¯ MnO4 + 8H+ + 5e¯ Li K Ca Na Mg Al Zn Cr 1₂ + 2e™ Hg²+ + 2e¯ Ag+ + e Br₂ + 2e™ Cl₂ +2e= Au³+ + 3e¯ F₂ +2e= Standard Reduction Potential for Selected Half-Cells Cl₂ +2e= PbO₂ + HSO4 + 3H+ + 2e¯ Fe Cd Ni Sn Pb H₂ Cu 21- Hg Ag 2Br 2C1- Reduction Half-Reaction → Au 2F- Increasing strength as reducing agent; increasing ease of oxidation → Zn + 4OH™ Fe + 2OH™ H₂ + 2OH- Pb + SO4²- NO₂ + 2OH- Sn²+ Ag + Cl- 2Hg + 2Cl- → 40H™ Ni(OH)₂ + 2OH- H₂ASO3 + H₂O Fe²+ CI- + 2OH- NO + 2H₂O 2H₂O 2Cr³+ + 7H₂O Mn²+ + 4H₂O 2C1™ PbSO4 + 2H₂O -3.045 -2.925 -2.87 -2.714 -2.37 -1.66 -0.763 -0.74 -0.44 -0.403 -0.25 -0.14 -0.126 0.000 +0.337 +0.535 +0.789 +0.799 +1.08 +1.360 +1.50 +2.87 Increasing strength as reducing agent; increasing ease of oxidation (reference electrode) Standard Reduction Potential Eº (volts) -1.22 -0.877 -0.828 -0.356 +0.01 +0.15 +0.222 +0.27 +0.40 +0.49 +0.58 +0.771 +0.89 +0.96 +1.229 +1.33 +1.507 +1.360 +1.685
Transcribed Image Text:TABLE 21-2 Element Li K Ca Na Mg Al Zn Cr Fe 2 3 2 5 2 3 2 2 3 2 Cd Ni Sn Pb 1₂ Hg Ag Br₂ Cl₂ Au F₂ TABLE 21-3 reduction of Increasing strength as oxidizing agent; ease increasing Just Buraptxo se Buons Butstanbu Standard Aqueous Reduction Potentials in Aqueous Solution at 25°C Standard Reduction Potential E (volts) increasing ease of reduction Reduction Half-Reaction Lit + e K+ + e¯ Ca²+ + 2e¯ Na+ + e- 2+ Mg²+ + 2e Al³+ + 3e¯ Zn²+ + 2e- Cr³+ + 3e¯ Fe²+ + 2e¯ Cd²+ + 2e- Ni²+ + 2e Sn²+ + 2e¯ Pb²+ 2e 2H+ + 2e™ Cu²+ + 2e¯ Zn(OH)4² +2e™ Fe(OH)₂ + 2e™ 2H₂O + 2e¯ PbSO4 + 2e¯ NO₂ + H₂O + 2e¯ 4+ Sn++ + 2e¯ AgCl + e Hg₂Cl₂ + 2e O₂ + 2H₂O + 4e¯ NiO₂ + 2H₂O + 2e¯ H₂AsO4 + 2H+ + 2e¯ 111 Fe³+ + e CIO + H₂O + 2e¯ NO₂ + 4H+ + 3e¯ O₂ + 4H+ + 4e¯ Cr₂O7²- + 14H+ + 6e¯ MnO4 + 8H+ + 5e¯ Li K Ca Na Mg Al Zn Cr 1₂ + 2e™ Hg²+ + 2e¯ Ag+ + e Br₂ + 2e™ Cl₂ +2e= Au³+ + 3e¯ F₂ +2e= Standard Reduction Potential for Selected Half-Cells Cl₂ +2e= PbO₂ + HSO4 + 3H+ + 2e¯ Fe Cd Ni Sn Pb H₂ Cu 21- Hg Ag 2Br 2C1- Reduction Half-Reaction → Au 2F- Increasing strength as reducing agent; increasing ease of oxidation → Zn + 4OH™ Fe + 2OH™ H₂ + 2OH- Pb + SO4²- NO₂ + 2OH- Sn²+ Ag + Cl- 2Hg + 2Cl- → 40H™ Ni(OH)₂ + 2OH- H₂ASO3 + H₂O Fe²+ CI- + 2OH- NO + 2H₂O 2H₂O 2Cr³+ + 7H₂O Mn²+ + 4H₂O 2C1™ PbSO4 + 2H₂O -3.045 -2.925 -2.87 -2.714 -2.37 -1.66 -0.763 -0.74 -0.44 -0.403 -0.25 -0.14 -0.126 0.000 +0.337 +0.535 +0.789 +0.799 +1.08 +1.360 +1.50 +2.87 Increasing strength as reducing agent; increasing ease of oxidation (reference electrode) Standard Reduction Potential Eº (volts) -1.22 -0.877 -0.828 -0.356 +0.01 +0.15 +0.222 +0.27 +0.40 +0.49 +0.58 +0.771 +0.89 +0.96 +1.229 +1.33 +1.507 +1.360 +1.685
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