Enter electrons as e-. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Al metal is put into a 1M aqueous Sn2+ solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. + + Standard Reduction (Electrode) Potentials at 25 oC Half-Cell ReactionEo (volts) Standard Reduction (Electrode) Potentials at 25 oC Standard Reduction (Electrode) Potentials at 25 oC Half-Cell ReactionEo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell ReactionEo (volts)F2(g) + 2 e- 2 F-(aq)2.87 Ce4+(aq) + e- Ce3+(aq)1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l)1.51 Cl2(g) + 2 e- 2 Cl-(aq)1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l)1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l)1.229Br2(l) + 2 e- 2 Br-(aq)1.08 NO3-(aq) + 4 H+(aq) + 3 e- NO(g) + 2 H2O(l)0.962 Hg2+(aq) + 2 e- Hg22+(aq)0.920 Hg2+(aq) + 2 e- Hg(l)0.855 Ag+(aq) + e- Ag(s)0.799 Hg22+(aq) + 2 e- 2 Hg(l)0.789 Fe3+(aq) + e- Fe2+(aq)0.771 I2(s) + 2 e- 2 I-(aq)0.535 Fe(CN)63-(aq) + e- Fe(CN)64-(aq)0.48 Cu2+(aq) + 2 e- Cu(s)0.337 Cu2+(aq) + e- Cu+(aq)0.153 S(s) + 2 H+(aq) + 2 e- H2S(aq)0.142 H+(aq) + 2 e- H2(g)0.0000Pb2+(aq) + 2 e- Pb(s)-0.126 Sn2+(aq) + 2 e- Sn(s)-0.14 Ni2+(aq) + 2 e- Ni(s)-0.25 Co2+(aq) + 2 e- Co(s)-0.28 Cd2+(aq) + 2 e- Cd(s)-0.403 Cr3+(aq) + e- Cr2+(aq)-0.41 Fe2+(aq) + 2 e- Fe(s)-0.44 Cr3+(aq) + 3 e- Cr(s)-0.74 Zn2+(aq) + 2 e- Zn(s)-0.7632 H2O(l) + 2 e- H2(g) + 2 OH-(aq)-0.83Mn2+(aq) + 2 e- Mn(s)-1.18Al3+(aq) + 3 e- Al(s)-1.66Mg2+(aq) + 2 e- Mg(s)-2.37Na+(aq) + e- Na(s)-2.714K+(aq) + e- K(s)-2.925Li+(aq) + e- Li(s)-3.045

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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Standard Reduction (Electrode) Potentials at 25 ^oC

Half-Cell ReactionE^o (volts)

Standard Reduction (Electrode) Potentials at 25 ^oC

Half-Cell ReactionE^o (volts)

Standard Reduction (Electrode) Potentials at 25 ^oC

Half-Cell ReactionE^o (volts)F₂(g) + 2 e^- 2 F^-(aq)2.87

Ce⁴⁺(aq) + e^- Ce³⁺(aq)1.61

MnO₄^-(aq) + 8 H⁺(aq) + 5 e^- Mn²⁺(aq) + 4 H₂O(l)1.51

Cl₂(g) + 2 e^- 2 Cl^-(aq)1.36

Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- 2 Cr³⁺(aq) + 7 H₂O(l)1.33

O₂(g) + 4 H⁺(aq) + 4 e^- 2 H₂O(l)1.229Br₂(l) + 2 e^- 2 Br^-(aq)1.08

NO₃^-(aq) + 4 H⁺(aq) + 3 e^- NO(g) + 2 H₂O(l)0.962

Hg²⁺(aq) + 2 e^- Hg₂²⁺(aq)0.920

Hg²⁺(aq) + 2 e^- Hg(l)0.855

Ag⁺(aq) + e^- Ag(s)0.799

Hg₂²⁺(aq) + 2 e^- 2 Hg(l)0.789

Fe³⁺(aq) + e^- Fe²⁺(aq)0.771

I₂(s) + 2 e^- 2 I^-(aq)0.535

Fe(CN)₆^3-(aq) + e^- Fe(CN)₆^4-(aq)0.48

Cu²⁺(aq) + 2 e^- Cu(s)0.337

Cu²⁺(aq) + e^- Cu⁺(aq)0.153

S(s) + 2 H⁺(aq) + 2 e^- H₂S(aq)0.142

H⁺(aq) + 2 e^- H₂(g)0.0000Pb²⁺(aq) + 2 e^- Pb(s)-0.126

Sn²⁺(aq) + 2 e^- Sn(s)-0.14

Ni²⁺(aq) + 2 e^- Ni(s)-0.25

Co²⁺(aq) + 2 e^- Co(s)-0.28

Cd²⁺(aq) + 2 e^- Cd(s)-0.403

Cr³⁺(aq) + e^- Cr²⁺(aq)-0.41

Fe²⁺(aq) + 2 e^- Fe(s)-0.44

Cr³⁺(aq) + 3 e^- Cr(s)-0.74

Zn²⁺(aq) + 2 e^- Zn(s)-0.7632 H₂O(l) + 2 e^- H₂(g) + 2 OH^-(aq)-0.83Mn²⁺(aq) + 2 e^- Mn(s)-1.18Al³⁺(aq) + 3 e^- Al(s)-1.66Mg²⁺(aq) + 2 e^- Mg(s)-2.37Na⁺(aq) + e^- Na(s)-2.714K⁺(aq) + e^- K(s)-2.925Li⁺(aq) + e^- Li(s)-3.045

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