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identify the half-reaction and calculate the cell potential of the following reactions. The cell potential table is given. Your final answer is simply the cell potential value. Standard Reduction Potentials for Common Half-Reactions at 25°C REDUCTION HALF-REACTIONS F2+2e-2F Ered (V) 2.886 1.763 REDUCTION HALF-REACTIONS Eºred (V) Sn²+2e-Sn Ni²+2e-Ni -0.137 -0.257 H₂O2(aq) + 2H() +2e-→ 2H₂O PbO2)+SO()+ 4H() +20- PbSO4 + 2H₂O → 1.687 Co² +2e--Co) (4) -0.277 -0.356 -0.440 Aug+ 3e-Aus Cla+2e-2Ch Cr₂O(g) 14H(+6e- 2Cr³+7H₂O 1.520 1.360 1.330 PbSO4)2e → PbSO Fe(+2e-Fe -0.744 Cr³+3eCf) Zn²+2e-Zn 1.229 -0.763 1.065 2H₂O +2e-Hau+20H) -0.828 O2+ 4H+40° → 2H₂O Bra+2e-2Br(a) Aga+eAg Hg2(aq) +20+2Hg Mn +2e-Mn -1.182 -1.676 -2.357 Fee-Fe²( 120)+2e-21 (9) Cu²+2e → Cu(s) Sn+2e-Sn²) 2H+2e-H₂ Pb2+2e-Pb(s) 0.799 0.796 0.771 0.534 0.340 0.154 0.000 -0.125 A³(aq) + 30+ Al(s) Mg(+2e-Mg Na e-Na Ca²+2e-Ca Ba2e-Ba K+eKist Lig+Li -2.714 -2.840 -2.920 -2.924 -3.040 1. Mg(s) + Sn²+ (aq) 2. Cl2(g) + 2Br (ag) Mg²+ (aq) Sn(s) → 2Cl- (aq) + Br₂(1) → +

identify the half-reaction and calculate the cell potential of the following reactions. The cell potential table is given. Your final answer is simply the cell potential value. Standard Reduction Potentials for Common Half-Reactions at 25°C REDUCTION HALF-REACTIONS F2+2e-2F Ered (V) 2.886 1.763 REDUCTION HALF-REACTIONS Eºred (V) Sn²+2e-Sn Ni²+2e-Ni -0.137 -0.257 H₂O2(aq) + 2H() +2e-→ 2H₂O PbO2)+SO()+ 4H() +20- PbSO4 + 2H₂O → 1.687 Co² +2e--Co) (4) -0.277 -0.356 -0.440 Aug+ 3e-Aus Cla+2e-2Ch Cr₂O(g) 14H(+6e- 2Cr³+7H₂O 1.520 1.360 1.330 PbSO4)2e → PbSO Fe(+2e-Fe -0.744 Cr³+3eCf) Zn²+2e-Zn 1.229 -0.763 1.065 2H₂O +2e-Hau+20H) -0.828 O2+ 4H+40° → 2H₂O Bra+2e-2Br(a) Aga+eAg Hg2(aq) +20+2Hg Mn +2e-Mn -1.182 -1.676 -2.357 Fee-Fe²( 120)+2e-21 (9) Cu²+2e → Cu(s) Sn+2e-Sn²) 2H+2e-H₂ Pb2+2e-Pb(s) 0.799 0.796 0.771 0.534 0.340 0.154 0.000 -0.125 A³(aq) + 30+ Al(s) Mg(+2e-Mg Na e-Na Ca²+2e-Ca Ba2e-Ba K+eKist Lig+Li -2.714 -2.840 -2.920 -2.924 -3.040 1. Mg(s) + Sn²+ (aq) 2. Cl2(g) + 2Br (ag) Mg²+ (aq) Sn(s) → 2Cl- (aq) + Br₂(1) → +

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
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identify the half-reaction and calculate the cell potential of the following reactions. The cell potential table is given. Your final answer is simply the cell potential value. Standard Reduction Potentials for Common Half-Reactions at 25°C Eºred (V) 2.866 1.763 REDUCTION HALF-REACTIONS Eºred (V) Sn²+ (aq) + 2e-→ Sn(s) REDUCTION HALF-REACTIONS F2(g) + 2e- →2F-(aq) H₂O2(aq) + 2H+ (aq) + 2e- → 2H₂O PbO2(s) + SO₂2 (aq) + 4H+ (aq) + 2e- → PbSO4(s) + 2H₂O -0.137 Ni²+ (aq) + 2e- → Ni(s) -0.257 1.687 Co²+ (aq) + 2e- → Co(s) -0.277 Au³+ (aq) + 3e-→ Au(s) PbSO4(aq) + 2e- → Pb(s) + SO4²- (aq) -0.356 1.520 1.360 Cl2(g) + 2e- →2CH(aq) Fe²+ (aq) + 2e-→ Fe(s) -0.440 Cr₂O72 (aq) + 14H+ (aq) + 6e- → 1.330 Cr3+ (aq) + 3e- → Cr(s) -0.744 2Cr³+ (aq) + 7H₂O O2(g) + 4H*(aq) + 4e¯ → 2H₂O) 1.229 Zn²+ (aq) + 2e-→ Zn(s) -0.763 Br2() +2e → 2Br (aq) 1.065 2H₂O + 2e → H₂(g) + 2OH(aq) -0.828 Ag+ (aq) + e → Ag(s) 0.799 Mn²+ (aq) + 2e- → Mn(s) -1.182 Hg₂+ (aq) + 2e → 2Hg() 0.796 Al³+ (aq) + 3e- → Al(s) -1.676 0.771 Mg2+ (aq) + 2e- → Mg(s) -2.357 Fe³+ (aq) + e- → Fe²+ (aq) 12(s) + 2e → 21 (aq) 0.534 Na* (aq) + e- → Na(s) -2.714 0.340 Ca²+, (aq) -2.840 (aq) Cu²+ + 2e- → Cu(s) Sn4+ +2e- → Sn²+ (aq) 2H¹ (aq) + 2e → H₂(g) 0.154 Ba2+ -2.920 (aq) (aq) 0.000 K* (aq) + e- → K(s) -2.924 Pb²+ (aq) + 2e → Pb(s) -0.125 Li+ (aq) + e- → Li(s) -3.040 1. Mg(s) + Sn²+ (aq) 2. Cl2(g) + 2Br (ag) Sn(s) Mg²+ (aq) + 2Cl(aq) + Br2(1) + 2e- → Ca(s) + 2e- → Ba(s)
Transcribed Image Text:identify the half-reaction and calculate the cell potential of the following reactions. The cell potential table is given. Your final answer is simply the cell potential value. Standard Reduction Potentials for Common Half-Reactions at 25°C Eºred (V) 2.866 1.763 REDUCTION HALF-REACTIONS Eºred (V) Sn²+ (aq) + 2e-→ Sn(s) REDUCTION HALF-REACTIONS F2(g) + 2e- →2F-(aq) H₂O2(aq) + 2H+ (aq) + 2e- → 2H₂O PbO2(s) + SO₂2 (aq) + 4H+ (aq) + 2e- → PbSO4(s) + 2H₂O -0.137 Ni²+ (aq) + 2e- → Ni(s) -0.257 1.687 Co²+ (aq) + 2e- → Co(s) -0.277 Au³+ (aq) + 3e-→ Au(s) PbSO4(aq) + 2e- → Pb(s) + SO4²- (aq) -0.356 1.520 1.360 Cl2(g) + 2e- →2CH(aq) Fe²+ (aq) + 2e-→ Fe(s) -0.440 Cr₂O72 (aq) + 14H+ (aq) + 6e- → 1.330 Cr3+ (aq) + 3e- → Cr(s) -0.744 2Cr³+ (aq) + 7H₂O O2(g) + 4H*(aq) + 4e¯ → 2H₂O) 1.229 Zn²+ (aq) + 2e-→ Zn(s) -0.763 Br2() +2e → 2Br (aq) 1.065 2H₂O + 2e → H₂(g) + 2OH(aq) -0.828 Ag+ (aq) + e → Ag(s) 0.799 Mn²+ (aq) + 2e- → Mn(s) -1.182 Hg₂+ (aq) + 2e → 2Hg() 0.796 Al³+ (aq) + 3e- → Al(s) -1.676 0.771 Mg2+ (aq) + 2e- → Mg(s) -2.357 Fe³+ (aq) + e- → Fe²+ (aq) 12(s) + 2e → 21 (aq) 0.534 Na* (aq) + e- → Na(s) -2.714 0.340 Ca²+, (aq) -2.840 (aq) Cu²+ + 2e- → Cu(s) Sn4+ +2e- → Sn²+ (aq) 2H¹ (aq) + 2e → H₂(g) 0.154 Ba2+ -2.920 (aq) (aq) 0.000 K* (aq) + e- → K(s) -2.924 Pb²+ (aq) + 2e → Pb(s) -0.125 Li+ (aq) + e- → Li(s) -3.040 1. Mg(s) + Sn²+ (aq) 2. Cl2(g) + 2Br (ag) Sn(s) Mg²+ (aq) + 2Cl(aq) + Br2(1) + 2e- → Ca(s) + 2e- → Ba(s)
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