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Standard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s) -237 Na (aq) +e Na(s) -2714 K' (aq) +e K(3) -2925 Li'(aq) +e- LI(s) -3.045 References Use the References to access important values if needed for this question. Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co*|Co half cell (E°red = -0.280V) and a standard Zn²“|Zn half cell (E°red = -0.763V). The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Submit Answer

Standard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s) -237 Na (aq) +e Na(s) -2714 K' (aq) +e K(3) -2925 Li'(aq) +e- LI(s) -3.045 References Use the References to access important values if needed for this question. Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co*|Co half cell (E°red = -0.280V) and a standard Zn²“|Zn half cell (E°red = -0.763V). The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Submit Answer

Chemistry
Chemistry
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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
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Standard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s) -237 Na (aq) +e Na(s) -2714 K' (aq) +e K(3) -2925 Li'(aq) +e- LI(s) -3.045
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 Half-Cell Reaction * (volts) F2(8) + 2 e2F (aq) 287 Ce* (aq) +e Ce (aq) 1.61 Mn0, (aq) + BH'(aq) +5e Mn"( "(aq) + 4 H20(1) 1.51 Cla(g) +2e -2 C (aq) 1.36 Cr20, (aq) + 14 H'(aq) - 6e2 Cr*"(aq) + 7 H20() 1.33 Oz() + 4 H'(aq) + 4e2 H20(1) 1.229 Br20) + 2 e2 Br (aq) 1.08 NO3 (aq) + 4 H'(aq) + 3eNO(g) + 2 H20() Hg"(aq) 0.96 2 Hg (aq) + 2e 0.920 Hg"(aq) + 2 e- Hg(1) 0.855 Ag (aq) +e Ag(s) 0.799 Hg2" (aq) - 2e-2 Hg(1) 0.789 Fe" (aq) +e Fe"(ag) 0.771 12(s) + 2e 21 (aq) 0.535 Fe(CN)"(aq) + e Fe(CN), (aq) 0.48 Cu (aq) + 2eCu(s) 0.337 Cu"(aq) +e- Cu (aq) 0.153 S(s) + 2 H'(aq) + 2 e H2S(aq) 0.14 2H'(aq) + 2e-H2(8) 0.0000 Pb (aq) + 2e- Ph(s) -0126 Sn (aq) + 2 e Sn(s) -014 Ni (aq) + 2 e- Ni(s) -0.25 Co (aq) + 2 e Co(s) -0.28 "(aq) + 2e Cd(s) -0.403 Cr"(aq) +e "(aq) -041 Fe"(aq) + 2 e Fe(s) -044 Cr"(aq) +3e-Cr(s) -0.74 Zn"(aq) +2 e- Zn(s) -0.763 2 H20() +2e Hz(z) + 2 OH (aq) -0.83 Mn"(aq) + 2e - Mn(s) -1.18 A" (aq) + 3e- Al(s) -1.66 Mg (aq) + 2 e- Mg(s) -237 Na (aq) +e Na(s) -2714 K' (aq) +e K(3) -2925 Li'(aq) +e- LI(s) -3.045
References Use the References to access important values if needed for this question. Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co*|Co half cell (E°red = -0.280V) and a standard Zn²“|Zn half cell (E°red = -0.763V). The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Submit Answer
Transcribed Image Text:References Use the References to access important values if needed for this question. Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic cell is constructed from a standard Co*|Co half cell (E°red = -0.280V) and a standard Zn²“|Zn half cell (E°red = -0.763V). The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V. Submit Answer
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