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What is the Eocell value for the reaction represented by the following cell diagram? Pt(s) | O2(g) | H2O2(aq) || Cu2+(aq) | Cu(s)

What is the Eocell value for the reaction represented by the following cell diagram? Pt(s) | O2(g) | H2O2(aq) || Cu2+(aq) | Cu(s)

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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What is the Eocell value for the reaction represented by the following cell diagram?

Pt(s) | O2(g) | H2O2(aq) || Cu2+(aq) | Cu(s)

TABLE 20.1 Potentials at 25 °C Some Selected Standard Electrode (Reduction) Reduction Half-Reaction E°, V Acidic solution F2g) + 2 e → 2 F (aq) +2.866 O3(g) + 2 H*(aq) + 2 e¯ S2O3 (aq) + 2 e → 2 SO,? (aq) H2O2(aq) + 2 H*(aq) + 2 e¯ MnO4 (aq) + 8 H*(aq) + 5 e¯ PbO2(s) + 4 H*(aq) + 2 e¯ → Cl2(g) + 2 e¯ –→ 2 Cl(aq) Cr,O,² (aq) + 14 H*(aq) + 6 e¯ – MnO2(s) + 4 H*(aq) + 2 e¯ O2(g) + 4 H*(aq) + 4 e 2 IO3 (aq) + 12 H*(aq) + 10 e¯ → I2(s) + 6 H2O(1) Br2(1) + 2 e –→ 2 Br (aq) NO3 (aq) + 4H*(aq) + 3 e¯ → NO(g) + 2 H2O(1) Ag"(aq) + e¯ Fe*(aq) + e¯ → Fe2*(aq) O2(g) + 2 H*(aq) + 2 e¯ → H2O2(aq) I2(s) + 2 e Cu²*(aq) + 2 e¯→ Cu(s) So,? (aq) + 4 H*(aq) + 2 e¯ → Sn**(aq) + 2 e¯ S(s) + 2 H*(aq) + 2 e¯ 2 H*(aq) + 2 e Pb2"(aq) + 2 e Sn²*(aq) + 2 e- Fe2*(aq) + 2 e Zn2*(aq) + 2 e Al3*(aq) + 3 e – Mg2"(aq) + 2 e¯ → Na"(aq) + e¯ Ca²*(aq) + 2 e¯ → Ca(s) K*(aq) + e Li*(aq) + e → Li(s) • O2(g) + H2O(1) +2.075 +2.01 → 2 H2O(1) Mn2+(aq) + 4 H2O(1) Pb²*(aq) + 2 H20(1) +1.763 +1.51 +1.455 +1.358 → 2 Cr³*(aq) + 7 H20(1) Mn²*(aq) + 2 H20(1) +1.33 +1.23 2 H20(1) +1.229 +1.20 +1.065 +0.956 Ag(s) +0.800 +0.771 +0.695 21(aq) +0.535 +0.340 2 H20(1) + SO2(g) +0.17 Sn²*(aq) → H2S(g) H2(g) Pb(s) · Sn(s) Fe(s) → Zn(s) Al(s) ► Mg(s) → Na(s) +0.154 +0.14 -0.125 -0.137 -0.440 -0.763 -1.676 -2.356 -2.713 -2.84 → K(s) -2.924 -3.040 Basic solution O3(g) + H2O(1) + 2 e¯ OCI(aq) + H,0(1) + 2 e¯ O2(g) + 2 H20(1) + 4 e¯ 2 H20(1) + 2 e¯→ H2(g) + 2 OH (aq) O2(g) + 2 OH (aq) CI (aq) + 2 OH (aq) 4 ОН (аq) +1.246 +0.890 +0.401 -0.828
Transcribed Image Text:TABLE 20.1 Potentials at 25 °C Some Selected Standard Electrode (Reduction) Reduction Half-Reaction E°, V Acidic solution F2g) + 2 e → 2 F (aq) +2.866 O3(g) + 2 H*(aq) + 2 e¯ S2O3 (aq) + 2 e → 2 SO,? (aq) H2O2(aq) + 2 H*(aq) + 2 e¯ MnO4 (aq) + 8 H*(aq) + 5 e¯ PbO2(s) + 4 H*(aq) + 2 e¯ → Cl2(g) + 2 e¯ –→ 2 Cl(aq) Cr,O,² (aq) + 14 H*(aq) + 6 e¯ – MnO2(s) + 4 H*(aq) + 2 e¯ O2(g) + 4 H*(aq) + 4 e 2 IO3 (aq) + 12 H*(aq) + 10 e¯ → I2(s) + 6 H2O(1) Br2(1) + 2 e –→ 2 Br (aq) NO3 (aq) + 4H*(aq) + 3 e¯ → NO(g) + 2 H2O(1) Ag"(aq) + e¯ Fe*(aq) + e¯ → Fe2*(aq) O2(g) + 2 H*(aq) + 2 e¯ → H2O2(aq) I2(s) + 2 e Cu²*(aq) + 2 e¯→ Cu(s) So,? (aq) + 4 H*(aq) + 2 e¯ → Sn**(aq) + 2 e¯ S(s) + 2 H*(aq) + 2 e¯ 2 H*(aq) + 2 e Pb2"(aq) + 2 e Sn²*(aq) + 2 e- Fe2*(aq) + 2 e Zn2*(aq) + 2 e Al3*(aq) + 3 e – Mg2"(aq) + 2 e¯ → Na"(aq) + e¯ Ca²*(aq) + 2 e¯ → Ca(s) K*(aq) + e Li*(aq) + e → Li(s) • O2(g) + H2O(1) +2.075 +2.01 → 2 H2O(1) Mn2+(aq) + 4 H2O(1) Pb²*(aq) + 2 H20(1) +1.763 +1.51 +1.455 +1.358 → 2 Cr³*(aq) + 7 H20(1) Mn²*(aq) + 2 H20(1) +1.33 +1.23 2 H20(1) +1.229 +1.20 +1.065 +0.956 Ag(s) +0.800 +0.771 +0.695 21(aq) +0.535 +0.340 2 H20(1) + SO2(g) +0.17 Sn²*(aq) → H2S(g) H2(g) Pb(s) · Sn(s) Fe(s) → Zn(s) Al(s) ► Mg(s) → Na(s) +0.154 +0.14 -0.125 -0.137 -0.440 -0.763 -1.676 -2.356 -2.713 -2.84 → K(s) -2.924 -3.040 Basic solution O3(g) + H2O(1) + 2 e¯ OCI(aq) + H,0(1) + 2 e¯ O2(g) + 2 H20(1) + 4 e¯ 2 H20(1) + 2 e¯→ H2(g) + 2 OH (aq) O2(g) + 2 OH (aq) CI (aq) + 2 OH (aq) 4 ОН (аq) +1.246 +0.890 +0.401 -0.828
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