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4) Please consider the following galvanic cell setup: the cell is composed of a silver rod dipped into a silver nitrate solution connected (via a salt bridge) to a solution of a magnesium rod dipped into a magnesium chloride solution. (a) Calculate the standard cell potential. (b) Define the anode and cathode.

4) Please consider the following galvanic cell setup: the cell is composed of a silver rod dipped into a silver nitrate solution connected (via a salt bridge) to a solution of a magnesium rod dipped into a magnesium chloride solution. (a) Calculate the standard cell potential. (b) Define the anode and cathode.

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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
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Please answer the question in the picture labeled #4 parts a and b. I also included a table of values im not sure if you will need it or if it will be irrelevant
TABLE 18.1 Standard Electrode Potentlals at 25 °C Reduction Half-Reaction F) + 2 e E (V) + 2F (aq) Stronger oxidizing agent H202(aq) + 2 H*(aq) + 2 e 2.87 +2 H20(0 → PBSO«(s) + 2 H20(1) → Mn02(s) + 2 H20() - Mn*(aq) + 4 H20(1) Weaker reducing agent PbO2(s) + 4 H*(ag) + SO,²¯(aq) + 2 e Mn04 (aq) + 4 H*(aq) + 3 e Mno. (aq) + 8 H*(aq) + 5 e Au+(aq) + 3e Pb02(s) + 4 H*(aq) + 2 e 1.78 1.69 1.68 1.51 - Au(s) 1.50 - Pb2*(aq) + 2 H20() → 2 cr (aq) 2 C*(aq) + 7 H2O) 2 H20(1) Mn+(aq) + 2 H,01) + (aq) + 3 H20() 1.46 Cl2lg) + 2 e Cr30, (aq) + 14 H*(aq) + 6 e 02(g) + 4 H*(aq) + 4 e MnO2(s) + 4 H*(aq) + 2 e 10, (aq) + 6 H*(aq) + 5 e Br() + 2 e Vo,"(aq) + 2 H*(aq) + e NO, (aq) + 4 H*(aq) + 3 e- 1.36 1.33 → 1.23 1.21 1.20 → 2 Br (aq) 1.09 - vo?"(aq) + H20() NOE) + 2 H20(1) → CIO, (aq) 1.00 0.96 CIO2() + e Ag"(aq) + e Fe*(aq) + e 0.95 Ag(s) + Fe?*(aq) 0.80 0.77 02(g) + 2 H*(aq) + 2 e Mno, (aq) +e b(s) + 2 e Cu*(aq) + e +H2O2(aq) 0.70 → Mn0,2 (aq) →21 (aq) → Cu(s) 4 OH (aq) + Cu(s) → H2SO3(aq) + H20(1) - Cu*(aq) - Sn*(aq) 0.56 0.54 0.52 02g) + 2 H20(1) + 4 e Cu*(aq) + 2 e 0.40 0.34 so, (aq) + 4 H*(aq) + 2 e Cu2*(aq) + e Snt(aq) + 2 e 2 H*(aq) + 2 e Fe(aq) + 3 e 0.20 0.16 0.15 - H2g) → Fe(s) → Pb(s) → Sn(s) -0.036 Pb2 (aq) + 2 e Sn2+(aq) + 2 e N2*(aq) + 2 e Cd*(aq) + 2 e Fe2+(aq) + 2 e Cr*(aq) + e Cr (aq) + 3 e Zn*(aq) + 2 e -0.13 -0.14 Ni(s) -0.23 → Cd(s) -0.40 - Fe(s) Cr2*(aq) -0.45 -0.50 - Cr(s) -0.73 + Zn(s) -0.76 + H2g) + 2 OH (aq) → Mn(s) + Al(s) -0.83 2 H20() + 2 e Mn2 (aq) + 2 e -1.18 -1.66 A*(aq) + 3 e Mg2+(aq) + 2 e Na (aq) + e Ca (aq) + 2 e Ba?+(aq) + 2 e K*(aq) + e oxidizing agent u*(aq) + e¯ -2.37 → Mg(s) → Na(s) -2.71 - Ca(s) -2.76 - Ba(s) -2.90 Stronger reducing agent - K(s) -2.92 Weaker - U(s) -3.04
Transcribed Image Text:TABLE 18.1 Standard Electrode Potentlals at 25 °C Reduction Half-Reaction F) + 2 e E (V) + 2F (aq) Stronger oxidizing agent H202(aq) + 2 H*(aq) + 2 e 2.87 +2 H20(0 → PBSO«(s) + 2 H20(1) → Mn02(s) + 2 H20() - Mn*(aq) + 4 H20(1) Weaker reducing agent PbO2(s) + 4 H*(ag) + SO,²¯(aq) + 2 e Mn04 (aq) + 4 H*(aq) + 3 e Mno. (aq) + 8 H*(aq) + 5 e Au+(aq) + 3e Pb02(s) + 4 H*(aq) + 2 e 1.78 1.69 1.68 1.51 - Au(s) 1.50 - Pb2*(aq) + 2 H20() → 2 cr (aq) 2 C*(aq) + 7 H2O) 2 H20(1) Mn+(aq) + 2 H,01) + (aq) + 3 H20() 1.46 Cl2lg) + 2 e Cr30, (aq) + 14 H*(aq) + 6 e 02(g) + 4 H*(aq) + 4 e MnO2(s) + 4 H*(aq) + 2 e 10, (aq) + 6 H*(aq) + 5 e Br() + 2 e Vo,"(aq) + 2 H*(aq) + e NO, (aq) + 4 H*(aq) + 3 e- 1.36 1.33 → 1.23 1.21 1.20 → 2 Br (aq) 1.09 - vo?"(aq) + H20() NOE) + 2 H20(1) → CIO, (aq) 1.00 0.96 CIO2() + e Ag"(aq) + e Fe*(aq) + e 0.95 Ag(s) + Fe?*(aq) 0.80 0.77 02(g) + 2 H*(aq) + 2 e Mno, (aq) +e b(s) + 2 e Cu*(aq) + e +H2O2(aq) 0.70 → Mn0,2 (aq) →21 (aq) → Cu(s) 4 OH (aq) + Cu(s) → H2SO3(aq) + H20(1) - Cu*(aq) - Sn*(aq) 0.56 0.54 0.52 02g) + 2 H20(1) + 4 e Cu*(aq) + 2 e 0.40 0.34 so, (aq) + 4 H*(aq) + 2 e Cu2*(aq) + e Snt(aq) + 2 e 2 H*(aq) + 2 e Fe(aq) + 3 e 0.20 0.16 0.15 - H2g) → Fe(s) → Pb(s) → Sn(s) -0.036 Pb2 (aq) + 2 e Sn2+(aq) + 2 e N2*(aq) + 2 e Cd*(aq) + 2 e Fe2+(aq) + 2 e Cr*(aq) + e Cr (aq) + 3 e Zn*(aq) + 2 e -0.13 -0.14 Ni(s) -0.23 → Cd(s) -0.40 - Fe(s) Cr2*(aq) -0.45 -0.50 - Cr(s) -0.73 + Zn(s) -0.76 + H2g) + 2 OH (aq) → Mn(s) + Al(s) -0.83 2 H20() + 2 e Mn2 (aq) + 2 e -1.18 -1.66 A*(aq) + 3 e Mg2+(aq) + 2 e Na (aq) + e Ca (aq) + 2 e Ba?+(aq) + 2 e K*(aq) + e oxidizing agent u*(aq) + e¯ -2.37 → Mg(s) → Na(s) -2.71 - Ca(s) -2.76 - Ba(s) -2.90 Stronger reducing agent - K(s) -2.92 Weaker - U(s) -3.04
4) Please consider the following galvanic cell setup: the cell is composed of a silver rod dipped into a silver nitrate solution connected (via a salt bridge) to a solution of a magnesium rod dipped into a magnesium chloride solution. (a) Calculate the standard cell potential. (b) Define the anode and cathode.
Transcribed Image Text:4) Please consider the following galvanic cell setup: the cell is composed of a silver rod dipped into a silver nitrate solution connected (via a salt bridge) to a solution of a magnesium rod dipped into a magnesium chloride solution. (a) Calculate the standard cell potential. (b) Define the anode and cathode.
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