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The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2*(aq) → Zn2+(aq) + Cu(s) Calculate the cell potential if the concentration of Zn2+ is 0.207 M and the concentration of Cu2+ is 1.488 M using the Nernst equation. E 0.0592 V Vlog Q

The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2*(aq) → Zn2+(aq) + Cu(s) Calculate the cell potential if the concentration of Zn2+ is 0.207 M and the concentration of Cu2+ is 1.488 M using the Nernst equation. E 0.0592 V Vlog Q

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
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The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2*(aq) → Zn2*(aq) + Cu(s) Calculate the cell potential if the concentration of Zn²+ is 0.207 M and the concentration of Cu2+ is 1.488 M using the Nernst equation. 0.0592 V E E° -log Q n
Transcribed Image Text:The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2*(aq) → Zn2*(aq) + Cu(s) Calculate the cell potential if the concentration of Zn²+ is 0.207 M and the concentration of Cu2+ is 1.488 M using the Nernst equation. 0.0592 V E E° -log Q n
Table 20.1 Standard Reduction Potentials in Water at 25 °C Efed (V) Reduction Half-Reaction +2.87 F2(g) + 2 e → 2F (aq) Mn²*(aq) + 4 H,O(1) MnO, (aq) + 8 H"(aq) + 5 e → 2 CF (aq) Cr,0,-(aq) + 14 H*(aq) + 6 e +1.51 +1.36 Cl,(8) + 2 e > +1.33 2 Cr* (aq) + 7 H,O(1) > +1.23 O2(g) + 4 H* (aq) + 4 e 2 H,0(1) > Br,(1) + 2 e NO, (aq) + 4 H*(aq) + 3 e Ag*(aq) + e Fe* (aq) + e +1.06 2 Br (aq) +0.96 NO(g) + 2 H,O(1) +0.80 Ag(s) +0.77 Fe2* (aq) +0.68 O2(g) + 2 H*(aq) + 2 e H,O2(aq) > +0.59 MnO, (aq) + 2 H,O(1) + 3 e MnO2(s) + 4 OH(aq) +0.54 2(s) + 2 e 21(aq) +0.40 O2(g) + 2 H,O(1) + 4 e –→ 4ОН (ад) +0.34 Cư*(aq) + 2 e 2H' (ад) + 2 е Cu(s) 0 [defined] H2(g) -0.28 Ni*(aq) + 2 e Ni(s) > -0.44 Fe2+ (aq) + 2 e Fe(s) - -0.76 Zn+(aq) + 2 e Zn(s) -0.83 2 H,O(1) + 2 e H2(g) + 2 OH (aq) -1.66 AB+(aq) + 3 e Al(s) > -2.71 Na" (aq) + e Na(s) -3.05 Li"(aq) + e Li(s) >
Transcribed Image Text:Table 20.1 Standard Reduction Potentials in Water at 25 °C Efed (V) Reduction Half-Reaction +2.87 F2(g) + 2 e → 2F (aq) Mn²*(aq) + 4 H,O(1) MnO, (aq) + 8 H"(aq) + 5 e → 2 CF (aq) Cr,0,-(aq) + 14 H*(aq) + 6 e +1.51 +1.36 Cl,(8) + 2 e > +1.33 2 Cr* (aq) + 7 H,O(1) > +1.23 O2(g) + 4 H* (aq) + 4 e 2 H,0(1) > Br,(1) + 2 e NO, (aq) + 4 H*(aq) + 3 e Ag*(aq) + e Fe* (aq) + e +1.06 2 Br (aq) +0.96 NO(g) + 2 H,O(1) +0.80 Ag(s) +0.77 Fe2* (aq) +0.68 O2(g) + 2 H*(aq) + 2 e H,O2(aq) > +0.59 MnO, (aq) + 2 H,O(1) + 3 e MnO2(s) + 4 OH(aq) +0.54 2(s) + 2 e 21(aq) +0.40 O2(g) + 2 H,O(1) + 4 e –→ 4ОН (ад) +0.34 Cư*(aq) + 2 e 2H' (ад) + 2 е Cu(s) 0 [defined] H2(g) -0.28 Ni*(aq) + 2 e Ni(s) > -0.44 Fe2+ (aq) + 2 e Fe(s) - -0.76 Zn+(aq) + 2 e Zn(s) -0.83 2 H,O(1) + 2 e H2(g) + 2 OH (aq) -1.66 AB+(aq) + 3 e Al(s) > -2.71 Na" (aq) + e Na(s) -3.05 Li"(aq) + e Li(s) >
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