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Calculate the standard cell potential for the following electrochemical reaction. Use the values from Table 20.1 (p .909) in the text. Mn2+(aq) + Sn2+(aq) Mn(s) + Snª+(aq)

Calculate the standard cell potential for the following electrochemical reaction. Use the values from Table 20.1 (p .909) in the text. Mn2+(aq) + Sn2+(aq) Mn(s) + Snª+(aq)

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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Calculate the standard cell potential for the following electrochemical reaction. Use the values from Table 20.1 (p .909) in the text. Mn2+(aq) + Sn²+(aq) Mn(s) + Snª+(aq) Answer:
Transcribed Image Text:Calculate the standard cell potential for the following electrochemical reaction. Use the values from Table 20.1 (p .909) in the text. Mn2+(aq) + Sn²+(aq) Mn(s) + Snª+(aq) Answer:
10:59 AM Wed Apr 13 令 2% 88 Chemistry - A Molecular Approach 4th ed - Nivaldo J. Tro (Pearson-1 - X CHM 1450 CH 19 Live Lecture Notes... CH 18 Live Lecture Notes (W22)-1 Untitled Notebook (2) Untitled Notebook (3) Chemistry - A Molecular Approac... . TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E°(V) F2(g) + 2 e 2 F (aq) 2.87 Weaker Stronger oxidizing agent H,0,(aq) + 2 H*(aq) + 2 e 2 H20(1) 1.78 reducing agent PbO,(s) + 4 H*(aq) + SO,²-(ag) + 2 e PbSO,(s) + 2 H,0(1) 1.69 Mn04 (aq) + 4 H*(aq) + 3 e¯ MnO2(s) + 2 H20(1) 1.68 Mno4 (aq) + 8 H*(aq) + 5 e Mn2+ (aq) + 4 H20(1) 1.51 Au3 + (aq) + 3 e Au(s) 1.50 PbO2(s) + 4 H*(aq) + 2 e Pb2+ (aq) + 2 H,0(1) 1.46 Cl2(g) + 2 e 2 СГ (ag) 1.36 Cr20,2-(aq) + 14 H*(aq) + 6 e 2 Cr3+ (aq) + 7 H20(1) 1.33 O2(g) + 4 H*(aq) + 4 e → 2 H20(I) 1.23 Mn02(s) + 4 H*(aq) + 2 e Mn2+ (aq) + 2 H,0(I) 1.21 2(aq) + 3 H,0(I) 2 Br (aq) 103 (aq) + 6 H*(aq) + 5 e 1.20 Br,(1) + 2 e 1.09 VO,*(aq) + 2 H*(aq) + e vo2+ (aq) + H20(1) 1.00 NO3 (aq) + 4 H*(aq) + 3 e NO(g) + 2 H20(1) 0.96 CIO2 (aq) → Ag(s) CIO2(g) + e 0.95 Ag* (aq) + e 0.80 Fe3+ (aq) + e → Fe2 + (aq) 0.77 O2(g) + 2 H*(aq) + 2 e H2O2(aq) 0.70 Mn04 (aq) + e Mno,2 (aq) 0.56 1(s) + 2 e 2 1 (aq) 0.54 Cu*(aq) + e Cu(s) 0.52 02(g) + 2 H,O(1) + 4 e 4 ОН (аg) 0.40 Cu2+(ag) + 2 e Cu(s) 0.34 So,2-(aq) + 4 H*(aq) + 2 e H2SO3(aq) + H20(1) 0.20 Cu2+ (aq) + e → Cu*(aq) 0.16 Sn4+ (aq) + 2 e Sn2+ (aq) 0.15 2 H*(aq) + 2 e H2(g) Fe3+ (ag) + 3 e Fe(s) -0.036 Pb2+ (aq) + 2 e Pb(s) -0.13 Sn2+ (aq) + 2 e Sn(s) -0.14 Ni2+ (aq) + 2 e Ni(s) -0.23 Cd2+(aq) + 2 e Cd(s) -0.40 Fe2 + (ag) + 2 e Fe(s) -0.45 Cr3+ (aq) + e Cr2+ (aq) -0.50 Cr3+ (aq) + 3 e Cr(s) -0.73 Zn2+(aq) + 2 e » Zn(s) -0.76 2 H20(1) + 2 e » H2(g) + 2 OH (aq) -0.83 Mn2 +(aq) + 2 e Mn(s) -1.18 Al3+ (aq) + 3 e » Al(s) -1.66 Mg2 + (aq) + 2 e Mg(s) -2.37 Na*(aq) + e Na(s) -2.71 Са2+ (ag) + 2 е » Ca(s) -2.76 Ba?+(ag) + 2 e Ba(s) -2.90 K*(aq) + e → K(s) -2.92 Weaker Stronger reducing agent oxidizing agent Lit(aq) + e » Li(s) -3.04 940 of 1315 902 Chapter 19 Electrochemistry LAUMPICTA ImusIaIcs How to CaicurUTe the potctlal OT an Clectrochemical cell
Transcribed Image Text:10:59 AM Wed Apr 13 令 2% 88 Chemistry - A Molecular Approach 4th ed - Nivaldo J. Tro (Pearson-1 - X CHM 1450 CH 19 Live Lecture Notes... CH 18 Live Lecture Notes (W22)-1 Untitled Notebook (2) Untitled Notebook (3) Chemistry - A Molecular Approac... . TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E°(V) F2(g) + 2 e 2 F (aq) 2.87 Weaker Stronger oxidizing agent H,0,(aq) + 2 H*(aq) + 2 e 2 H20(1) 1.78 reducing agent PbO,(s) + 4 H*(aq) + SO,²-(ag) + 2 e PbSO,(s) + 2 H,0(1) 1.69 Mn04 (aq) + 4 H*(aq) + 3 e¯ MnO2(s) + 2 H20(1) 1.68 Mno4 (aq) + 8 H*(aq) + 5 e Mn2+ (aq) + 4 H20(1) 1.51 Au3 + (aq) + 3 e Au(s) 1.50 PbO2(s) + 4 H*(aq) + 2 e Pb2+ (aq) + 2 H,0(1) 1.46 Cl2(g) + 2 e 2 СГ (ag) 1.36 Cr20,2-(aq) + 14 H*(aq) + 6 e 2 Cr3+ (aq) + 7 H20(1) 1.33 O2(g) + 4 H*(aq) + 4 e → 2 H20(I) 1.23 Mn02(s) + 4 H*(aq) + 2 e Mn2+ (aq) + 2 H,0(I) 1.21 2(aq) + 3 H,0(I) 2 Br (aq) 103 (aq) + 6 H*(aq) + 5 e 1.20 Br,(1) + 2 e 1.09 VO,*(aq) + 2 H*(aq) + e vo2+ (aq) + H20(1) 1.00 NO3 (aq) + 4 H*(aq) + 3 e NO(g) + 2 H20(1) 0.96 CIO2 (aq) → Ag(s) CIO2(g) + e 0.95 Ag* (aq) + e 0.80 Fe3+ (aq) + e → Fe2 + (aq) 0.77 O2(g) + 2 H*(aq) + 2 e H2O2(aq) 0.70 Mn04 (aq) + e Mno,2 (aq) 0.56 1(s) + 2 e 2 1 (aq) 0.54 Cu*(aq) + e Cu(s) 0.52 02(g) + 2 H,O(1) + 4 e 4 ОН (аg) 0.40 Cu2+(ag) + 2 e Cu(s) 0.34 So,2-(aq) + 4 H*(aq) + 2 e H2SO3(aq) + H20(1) 0.20 Cu2+ (aq) + e → Cu*(aq) 0.16 Sn4+ (aq) + 2 e Sn2+ (aq) 0.15 2 H*(aq) + 2 e H2(g) Fe3+ (ag) + 3 e Fe(s) -0.036 Pb2+ (aq) + 2 e Pb(s) -0.13 Sn2+ (aq) + 2 e Sn(s) -0.14 Ni2+ (aq) + 2 e Ni(s) -0.23 Cd2+(aq) + 2 e Cd(s) -0.40 Fe2 + (ag) + 2 e Fe(s) -0.45 Cr3+ (aq) + e Cr2+ (aq) -0.50 Cr3+ (aq) + 3 e Cr(s) -0.73 Zn2+(aq) + 2 e » Zn(s) -0.76 2 H20(1) + 2 e » H2(g) + 2 OH (aq) -0.83 Mn2 +(aq) + 2 e Mn(s) -1.18 Al3+ (aq) + 3 e » Al(s) -1.66 Mg2 + (aq) + 2 e Mg(s) -2.37 Na*(aq) + e Na(s) -2.71 Са2+ (ag) + 2 е » Ca(s) -2.76 Ba?+(ag) + 2 e Ba(s) -2.90 K*(aq) + e → K(s) -2.92 Weaker Stronger reducing agent oxidizing agent Lit(aq) + e » Li(s) -3.04 940 of 1315 902 Chapter 19 Electrochemistry LAUMPICTA ImusIaIcs How to CaicurUTe the potctlal OT an Clectrochemical cell
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