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2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g)   a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures.

2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g)   a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section: Chapter Questions
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In an electrolysis of a solution with sodium chloride NaCl(aq), sodium hydroxide is formed NaOH(aq), chlorine gas Cl2(g), and hydrogen gas H2(g), after the reaction equation:
2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g)
 
a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures.
 
b) Use the table at the back of the task set and set up two half-reactions describing what is happening on the anode and cathode of this electrolysis. 
TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E° (V) F₂(g) + 2e →→→→2F (aq) +2.87 +2.07 O3(g) + 2H+ (aq) + 2eO₂(g) + H₂O Co³+ (aq) + e- Co²+ (aq) 3+ +1.82 H₂O₂(aq) + 2H+ (aq) + 2e → → 2H₂O +1.77 PbO₂ (s) + 4H+ (aq) + SO4 (aq) + 2ePbSO4(s) + 2H₂O +1.70 4+ 3+ Ce¹+ (aq) + e Ce³+ (aq) +1.61 2+ MnO, (aq) + 8H* (aq) + Se → Mn²+ (aq) + 4H₂O +1.51 3+ Au³+ (aq) + 3e. → Au(s) +1.50 Cl₂(g) + 2e →→→→→→→2Cl¯ (aq) +1.36 +1.33 2+ +1.23 +1.23 Cr₂O (aq) + 14H* (aq) + 6e7 →→2Cr³+ (aq) + 7H₂O MnO₂(s) + 4H+ (aq) + 2e7 →→Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e¯¯ →→→ 2H₂O Br₂() +2e7 →→→→2Br (aq) NO3(aq) + 4H+ (aq) + 3e¯ 2Hg²+ (aq) + 2e → Hg+ (aq) + 2e - +1.07 NO(g) + 2H₂O +0.96 Hg2+ (aq) +0.92 2Hg(1) +0.85 Ag(s) +0.80 >Fe²+ (aq) +0.77 > H₂O₂(aq) +0.68 Ag (aq) + e - Fe³+ (aq) + e O₂(g) + 2H+ (aq) + 2e¯ MnO4 (aq) + 2H₂O + 3e7 I₂(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e¯ Cu²+ (aq) + 2e → Cu(s) - MnO₂(s) + 4OH(aq) +0.59 +0.53 4OH(aq) +0.40 +0.34 AgCl(s) + e - Ag(s) + Cl(aq) +0.22 SO (aq) + 4H+ (aq) + 2e¯¯ > SO₂(g) + 2H₂O : +0.20 2+ +0.15 Cu²+ (aq) + e → Sn¹+ (aq) + 2e 2H(aq) + 2e7 Pb²+ (aq) + 2e7 Sn²+ (aq) + 2e7 Cu+ (aq) →→→→Sn²+ (aq) → H₂(g) +0.13 0.00 Pb(s) -0.13 Sn(s) -0.14 Ni²+ (aq) + 2e7 →→→→Ni(s) -0.25 → Co(s) -0.28 → Pb(s) + SO³(aq) -0.31 Co²+ (aq) + 2e PbSO4(s) + 2e7 Cd²+ (aq) + 2e Fe²+ (aq) + 2e7 -0.40 -Cd(s) → Fe(s) → Cr(s) -0.44 Cr³+ (aq) + 3e7 -0.74 Zn²+ (aq) + 2e →→→ Zn(s) -0.76 2H₂O + 2e →→→ H₂(g) + 2OH(aq) -0.83 2+ Mn²+ (aq) + 2e → Mn(s) -1.18 →Al(s) -1.66 Al³+ (aq) + 3e7 Be²+ (aq) + 2e → Be(s) -1.85 Mg²+ (aq) + 2e →→→→Mg(s) -2.37 Na (aq) + e →→→→Na(s) -2.71 -2.87 -2.89 Ca²+ (aq) + 2e7 → Ca(s) Sr²+ (aq) + 2e7 → Sr(s) Ba2+ (aq) + 2e7 →→→→Ba(s) K+ (aq) + e→→→→→→→K(s) Lit(aq) + e→→→→→→Li(s) -2.90 -2.93 -3.05 *For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard.state values Increasing strength as oxidizing ageni Increasing strength as reducing agent
Transcribed Image Text:TABLE 19.1 Standard Reduction Potentials at 25°C* Half-Reaction E° (V) F₂(g) + 2e →→→→2F (aq) +2.87 +2.07 O3(g) + 2H+ (aq) + 2eO₂(g) + H₂O Co³+ (aq) + e- Co²+ (aq) 3+ +1.82 H₂O₂(aq) + 2H+ (aq) + 2e → → 2H₂O +1.77 PbO₂ (s) + 4H+ (aq) + SO4 (aq) + 2ePbSO4(s) + 2H₂O +1.70 4+ 3+ Ce¹+ (aq) + e Ce³+ (aq) +1.61 2+ MnO, (aq) + 8H* (aq) + Se → Mn²+ (aq) + 4H₂O +1.51 3+ Au³+ (aq) + 3e. → Au(s) +1.50 Cl₂(g) + 2e →→→→→→→2Cl¯ (aq) +1.36 +1.33 2+ +1.23 +1.23 Cr₂O (aq) + 14H* (aq) + 6e7 →→2Cr³+ (aq) + 7H₂O MnO₂(s) + 4H+ (aq) + 2e7 →→Mn²+ (aq) + 2H₂O O₂(g) + 4H+ (aq) + 4e¯¯ →→→ 2H₂O Br₂() +2e7 →→→→2Br (aq) NO3(aq) + 4H+ (aq) + 3e¯ 2Hg²+ (aq) + 2e → Hg+ (aq) + 2e - +1.07 NO(g) + 2H₂O +0.96 Hg2+ (aq) +0.92 2Hg(1) +0.85 Ag(s) +0.80 >Fe²+ (aq) +0.77 > H₂O₂(aq) +0.68 Ag (aq) + e - Fe³+ (aq) + e O₂(g) + 2H+ (aq) + 2e¯ MnO4 (aq) + 2H₂O + 3e7 I₂(s) + 2e21 (aq) O₂(g) + 2H₂O + 4e¯ Cu²+ (aq) + 2e → Cu(s) - MnO₂(s) + 4OH(aq) +0.59 +0.53 4OH(aq) +0.40 +0.34 AgCl(s) + e - Ag(s) + Cl(aq) +0.22 SO (aq) + 4H+ (aq) + 2e¯¯ > SO₂(g) + 2H₂O : +0.20 2+ +0.15 Cu²+ (aq) + e → Sn¹+ (aq) + 2e 2H(aq) + 2e7 Pb²+ (aq) + 2e7 Sn²+ (aq) + 2e7 Cu+ (aq) →→→→Sn²+ (aq) → H₂(g) +0.13 0.00 Pb(s) -0.13 Sn(s) -0.14 Ni²+ (aq) + 2e7 →→→→Ni(s) -0.25 → Co(s) -0.28 → Pb(s) + SO³(aq) -0.31 Co²+ (aq) + 2e PbSO4(s) + 2e7 Cd²+ (aq) + 2e Fe²+ (aq) + 2e7 -0.40 -Cd(s) → Fe(s) → Cr(s) -0.44 Cr³+ (aq) + 3e7 -0.74 Zn²+ (aq) + 2e →→→ Zn(s) -0.76 2H₂O + 2e →→→ H₂(g) + 2OH(aq) -0.83 2+ Mn²+ (aq) + 2e → Mn(s) -1.18 →Al(s) -1.66 Al³+ (aq) + 3e7 Be²+ (aq) + 2e → Be(s) -1.85 Mg²+ (aq) + 2e →→→→Mg(s) -2.37 Na (aq) + e →→→→Na(s) -2.71 -2.87 -2.89 Ca²+ (aq) + 2e7 → Ca(s) Sr²+ (aq) + 2e7 → Sr(s) Ba2+ (aq) + 2e7 →→→→Ba(s) K+ (aq) + e→→→→→→→K(s) Lit(aq) + e→→→→→→Li(s) -2.90 -2.93 -3.05 *For all half-reactions the concentration is 1 M for dissolved species and the pressure is 1 atm for gases. These are the standard.state values Increasing strength as oxidizing ageni Increasing strength as reducing agent
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