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(1). Balance the following redox reaction in a basic solution and indicate which half-reaction is taking place at the cathode and which at the anode? CIO3(aq) + Br (aq) ---> Cl₂ (g) + Br₂ (1) (2) Calculate the standard emf (in Volts) for this voltaic cell? You must type the answer in the text box below. (3) sketch the voltaic cell. (show your work on paper)

(1). Balance the following redox reaction in a basic solution and indicate which half-reaction is taking place at the cathode and which at the anode? CIO3(aq) + Br (aq) ---> Cl₂ (g) + Br₂ (1) (2) Calculate the standard emf (in Volts) for this voltaic cell? You must type the answer in the text box below. (3) sketch the voltaic cell. (show your work on paper)

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.128QP: a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4...
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(1). Balance the following redox reaction in a basic solution and indicate which half-reaction is taking place at the cathode and which at the anode? CIO3(aq) + Br (aq) ---> Cl₂ (g) + Br₂ (1) (2) Calculate the standard emf (in Volts) for this voltaic cell? You must type the answer in the text box below. (3) sketch the voltaic cell. (show your work on paper)
Transcribed Image Text:(1). Balance the following redox reaction in a basic solution and indicate which half-reaction is taking place at the cathode and which at the anode? CIO3(aq) + Br (aq) ---> Cl₂ (g) + Br₂ (1) (2) Calculate the standard emf (in Volts) for this voltaic cell? You must type the answer in the text box below. (3) sketch the voltaic cell. (show your work on paper)
Half-Reaction Ag+ (aq) + e¯ Ag(s) Ag(s) + Br(aq) AgBr(s) + e AgCl(s) + e Ag(s) + Cl(aq) Ag(CN)₂ (aq) + e¯ Ag₂CrO4(s) + 2e¯ Agl(s) + e Ag(s) + 2 CN(aq) 2 Ag(s) + CrO2 (aq) Ag(s) + (aq) Ag(S₂O3)₂³(aq) + e¯ Ag(s) + 2S₂O3²¯¯(aq) Al³+ (aq) + 3 e Al(s) H3ASO4(aq) + 2H+ (aq) + 2e¯ 2+ Ba²+ (aq) + 2 e Ba(s) BIO+ (aq) + 2 H+ (aq) + 3 e Br₂(1) + 2 e → 2 Br (aq) 2 BrO3(aq) + 12 H(aq) + 10 e 2 CO₂(g) + 2 H+ (aq) + 2 e Ca²+ (aq) + 2 e Ca(s) Cd²+ (aq) + 2 e Cd(s) Ce³+ (aq) Ce+ (aq) + e Cl₂(g) + 2 e 2 Cl(aq) 2 HClO(aq) + 2H*(aq) +2e ClO (aq) + H,O(l) + 2e 2 ClO3(aq) + 12 H(aq) + 10 e Co²+ (aq) + 2 e - Co(s) Co³+ (aq) + e Co²+ (aq) Cr³+ (aq) + 3 e Cr(s) 3+ Cr³+ (aq) + e Cr²+ (aq) H3ASO3(aq) + H₂O(1) Bi(s) + H₂O(l) Br₂(1) + 6 H₂O(1) H₂C₂O4(aq) Cl₂(g) + 2 H₂O(1) Cl(aq) + 2OH(aq) Cl₂(g) + 6 H₂O(1) E°(V) +0.799 +0.095 +0.222 -0.31 +0.446 -0.151 +0.01 -1.66 +0.559 -2.90 +0.32 +1.065 +1.52 -0.49 -2.87 -0.403 +1.61 +1.359 +1.63 +0.89 +1.47 -0.277 +1.842 -0.74 -0.41 Half-Reaction 2 H₂O(l) + 2 e HO₂ (aq) + H₂O(l) + 2 e H₂O₂(aq) + 2 H+ (aq) 2+ Hg₂²+ (aq) + 2 e 2 Hg2+ (aq) + 2 e¯ Hg²+ (aq) + 2 e Hg(1) 1₂(s) + 2 e 21(aq) 2 103 (aq) + 12 H+ (aq) + 10 e K+ (aq) + e Lit(aq) + e¯ →→→→K(s) Li(s) 2+ Mg²+ (aq) + 2 e Mg(s) Mn²+ (aq) + 2 e Mn(s) MnO₂ (s) + 4H+ (aq) + 2 e¯ MnO4 (aq) + 8 H+ (aq) + 5 e MnO4 (aq) + 2 H₂O(l) + 3 e¯ HNO₂(aq) + H*(aq) + e¯ N₂(g) + 4H₂O(l) + 4e¯ →→ N₂(g) + 5 H(aq) + 4e¯ NO3(aq) + 4H+ (aq) + 3 e¯ Na+ (aq) + e Na(s) Ni²+ (aq) + 2 e Ni(s) O₂(g) + 4H+ (aq) + 4e¯ →→ 2 H₂O(1) 4 OH(aq) O₂(g) + 2 H₂O(l) + 4e¯ Oz(g) + 2H*(aq) + 2 e H₂O₂(aq) O3(g) + 2 H+ (aq) + 2 e¯→→→→→→ O₂(g) + H₂O(1) DL2+( Dh() H₂(g) + 2 OH(aq) + 2 e¯ 3 OH(aq) 2 H₂O(1) 2 Hg(1) 2+ Hg₂²+ (aq) 1₂(s) + 6 H₂O(1) 2+ Mn²+ (aq) + 2 H₂O(l) 2+ Mn²+ (aq) + 4H₂O(1) MnO₂ (s) + 4 OH(aq) NO(g) + H₂O(1) 4 OH¯(aq) + N₂H₂(aq) N₂H5+ (aq) NO(g) + 2 H₂O(1) E°(V) -0.83 +0.88 +1.776 +0.789 +0.920 +0.854 +0.536 +1.195 -2.925 -3.05 -2.37 -1.18 +1.23 +1.51 +0.59 +1.00 -1.16 -0.23 +0.96 -2.71 -0.28 +1.23 +0.40 +0.68 +2.07 012
Transcribed Image Text:Half-Reaction Ag+ (aq) + e¯ Ag(s) Ag(s) + Br(aq) AgBr(s) + e AgCl(s) + e Ag(s) + Cl(aq) Ag(CN)₂ (aq) + e¯ Ag₂CrO4(s) + 2e¯ Agl(s) + e Ag(s) + 2 CN(aq) 2 Ag(s) + CrO2 (aq) Ag(s) + (aq) Ag(S₂O3)₂³(aq) + e¯ Ag(s) + 2S₂O3²¯¯(aq) Al³+ (aq) + 3 e Al(s) H3ASO4(aq) + 2H+ (aq) + 2e¯ 2+ Ba²+ (aq) + 2 e Ba(s) BIO+ (aq) + 2 H+ (aq) + 3 e Br₂(1) + 2 e → 2 Br (aq) 2 BrO3(aq) + 12 H(aq) + 10 e 2 CO₂(g) + 2 H+ (aq) + 2 e Ca²+ (aq) + 2 e Ca(s) Cd²+ (aq) + 2 e Cd(s) Ce³+ (aq) Ce+ (aq) + e Cl₂(g) + 2 e 2 Cl(aq) 2 HClO(aq) + 2H*(aq) +2e ClO (aq) + H,O(l) + 2e 2 ClO3(aq) + 12 H(aq) + 10 e Co²+ (aq) + 2 e - Co(s) Co³+ (aq) + e Co²+ (aq) Cr³+ (aq) + 3 e Cr(s) 3+ Cr³+ (aq) + e Cr²+ (aq) H3ASO3(aq) + H₂O(1) Bi(s) + H₂O(l) Br₂(1) + 6 H₂O(1) H₂C₂O4(aq) Cl₂(g) + 2 H₂O(1) Cl(aq) + 2OH(aq) Cl₂(g) + 6 H₂O(1) E°(V) +0.799 +0.095 +0.222 -0.31 +0.446 -0.151 +0.01 -1.66 +0.559 -2.90 +0.32 +1.065 +1.52 -0.49 -2.87 -0.403 +1.61 +1.359 +1.63 +0.89 +1.47 -0.277 +1.842 -0.74 -0.41 Half-Reaction 2 H₂O(l) + 2 e HO₂ (aq) + H₂O(l) + 2 e H₂O₂(aq) + 2 H+ (aq) 2+ Hg₂²+ (aq) + 2 e 2 Hg2+ (aq) + 2 e¯ Hg²+ (aq) + 2 e Hg(1) 1₂(s) + 2 e 21(aq) 2 103 (aq) + 12 H+ (aq) + 10 e K+ (aq) + e Lit(aq) + e¯ →→→→K(s) Li(s) 2+ Mg²+ (aq) + 2 e Mg(s) Mn²+ (aq) + 2 e Mn(s) MnO₂ (s) + 4H+ (aq) + 2 e¯ MnO4 (aq) + 8 H+ (aq) + 5 e MnO4 (aq) + 2 H₂O(l) + 3 e¯ HNO₂(aq) + H*(aq) + e¯ N₂(g) + 4H₂O(l) + 4e¯ →→ N₂(g) + 5 H(aq) + 4e¯ NO3(aq) + 4H+ (aq) + 3 e¯ Na+ (aq) + e Na(s) Ni²+ (aq) + 2 e Ni(s) O₂(g) + 4H+ (aq) + 4e¯ →→ 2 H₂O(1) 4 OH(aq) O₂(g) + 2 H₂O(l) + 4e¯ Oz(g) + 2H*(aq) + 2 e H₂O₂(aq) O3(g) + 2 H+ (aq) + 2 e¯→→→→→→ O₂(g) + H₂O(1) DL2+( Dh() H₂(g) + 2 OH(aq) + 2 e¯ 3 OH(aq) 2 H₂O(1) 2 Hg(1) 2+ Hg₂²+ (aq) 1₂(s) + 6 H₂O(1) 2+ Mn²+ (aq) + 2 H₂O(l) 2+ Mn²+ (aq) + 4H₂O(1) MnO₂ (s) + 4 OH(aq) NO(g) + H₂O(1) 4 OH¯(aq) + N₂H₂(aq) N₂H5+ (aq) NO(g) + 2 H₂O(1) E°(V) -0.83 +0.88 +1.776 +0.789 +0.920 +0.854 +0.536 +1.195 -2.925 -3.05 -2.37 -1.18 +1.23 +1.51 +0.59 +1.00 -1.16 -0.23 +0.96 -2.71 -0.28 +1.23 +0.40 +0.68 +2.07 012
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