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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.

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter19: Applications Of Standard Electrode Potentials
Section: Chapter Questions
Problem 19.8QAP
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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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