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Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and F2​(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.  Fill 4 blanks ____

Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and F2​(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.  Fill 4 blanks ____

Chemistry
Chemistry
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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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and F2​(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.  Fill 4 blanks ____
Standard Reduction (Electrode) Potentials at 25 °C Cu2+(a *(aq) + 2 e →→→→Cu(s) Cu²+ (aq) + e →→→→Cu* (aq) S(s) + 2 H+ (aq) + 2 e² →→→→ H₂S(aq) 2 H(aq) + 2 e →→→ H₂(g) (aq) + 2 e Pb(s) → Sn²+ (aq) + 2 e→→→→→→Sn(s) Ni2+ (aq) + 2 e² →→→→→→Ni(s) Co2+ (aq) + 2 e. Co(s) → Cd2+ (aq) + 2 e- Cd(s) Cr³+ (aq) + e- Cr²+ (aq) e2+ (aq) + 2 e Fe(s) Cr³+ (aq) + 3 e →→→ Cr(s) Zn²+ (aq) + 2 e- Zn(s) → 2 H₂O(l) +2e →→→→ H₂(g) + 2 OH(aq) Pb2+( Fe2+ Half-Cell Reaction → Mn²+ (aq) +2 e- →→→→Mn(s) A1³+ (aq) + 3 e²Al(s) Mg2+ (aq) + 2 e→→→→→→ Mg(s) Eº (volts) 0.337 0.153 0.14 0.0000 -0.126 -0.14 -0.25 -0.28 -0.403 -0.41 -0.44 -0.74 -0.763 -0.83 -1.18 -1.66 -2.37
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Cu2+(a *(aq) + 2 e →→→→Cu(s) Cu²+ (aq) + e →→→→Cu* (aq) S(s) + 2 H+ (aq) + 2 e² →→→→ H₂S(aq) 2 H(aq) + 2 e →→→ H₂(g) (aq) + 2 e Pb(s) → Sn²+ (aq) + 2 e→→→→→→Sn(s) Ni2+ (aq) + 2 e² →→→→→→Ni(s) Co2+ (aq) + 2 e. Co(s) → Cd2+ (aq) + 2 e- Cd(s) Cr³+ (aq) + e- Cr²+ (aq) e2+ (aq) + 2 e Fe(s) Cr³+ (aq) + 3 e →→→ Cr(s) Zn²+ (aq) + 2 e- Zn(s) → 2 H₂O(l) +2e →→→→ H₂(g) + 2 OH(aq) Pb2+( Fe2+ Half-Cell Reaction → Mn²+ (aq) +2 e- →→→→Mn(s) A1³+ (aq) + 3 e²Al(s) Mg2+ (aq) + 2 e→→→→→→ Mg(s) Eº (volts) 0.337 0.153 0.14 0.0000 -0.126 -0.14 -0.25 -0.28 -0.403 -0.41 -0.44 -0.74 -0.763 -0.83 -1.18 -1.66 -2.37
Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction F₂(g) +2 e 2 F"(aq) Ce4+ (aq) + eCe³+ (aq) MnO4 (aq) + 8 H(aq) + 5 e- —Mn2+(aq)+4 H,O(1) Cl₂(g) +2 e 2 Cl(aq) Cr₂O2(aq) + 14 H(aq) + 6 e² →→→ 2 Cr³+ (aq) + 7 H₂O(1) O₂(g) + 4 H*(aq) + 4e → 2 H₂O(1) Br₂(1) +2 e2 Br(aq) NO3(aq) + 4 H¹ (aq) + 3 e¯ →→→ NO(g) + 2 H₂O(1) 2 Hg2+ (aq) + 2 e →→→→→Hg₂²+ (aq) Hg2+ (aq) + 2 e →→→→Hg(1) Ag (aq) + e- →→→→→Ag(s) Hg₂ ₂2+ (aq) + 2 e- → 2 Hg(1) Fe³+ (aq) + e Fe²+ (aq) → 1₂(s) +2 e 2 I¯ (aq) → Fe(CN)6³(aq) + e→→→→→→Fe(CN)6+ (aq) Eº (volts) 2.87 1.61 1.51 1.36 1.33 1.229 1.08 0.96 0.920 0.855 0.799 0.789 0.771 0.535 0.48
Transcribed Image Text:Standard Reduction (Electrode) Potentials at 25 °C Half-Cell Reaction F₂(g) +2 e 2 F"(aq) Ce4+ (aq) + eCe³+ (aq) MnO4 (aq) + 8 H(aq) + 5 e- —Mn2+(aq)+4 H,O(1) Cl₂(g) +2 e 2 Cl(aq) Cr₂O2(aq) + 14 H(aq) + 6 e² →→→ 2 Cr³+ (aq) + 7 H₂O(1) O₂(g) + 4 H*(aq) + 4e → 2 H₂O(1) Br₂(1) +2 e2 Br(aq) NO3(aq) + 4 H¹ (aq) + 3 e¯ →→→ NO(g) + 2 H₂O(1) 2 Hg2+ (aq) + 2 e →→→→→Hg₂²+ (aq) Hg2+ (aq) + 2 e →→→→Hg(1) Ag (aq) + e- →→→→→Ag(s) Hg₂ ₂2+ (aq) + 2 e- → 2 Hg(1) Fe³+ (aq) + e Fe²+ (aq) → 1₂(s) +2 e 2 I¯ (aq) → Fe(CN)6³(aq) + e→→→→→→Fe(CN)6+ (aq) Eº (volts) 2.87 1.61 1.51 1.36 1.33 1.229 1.08 0.96 0.920 0.855 0.799 0.789 0.771 0.535 0.48
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