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Calculate AG and the equilibrium constant for the following reaction at 298 K: Zn²+ (aq) + Ni(s) → Zn(s) + Ni²+ (aq) Acidic Solution Standard Electrode Potential, E (volts) 2 H₂O(l) +1.77 H₂O₂(aq) + 2 H*(aq) + 2 e Au*(aq) + e — Au(s) +1.68 Au3(aq) + 3e — Au(s) +1.50 Br₂(l) +2 e 2 Br(aq) +1.08 NO3(aq) + 4 H*(aq) + 3 e NO(g) + 2 H₂O +0.96 Ag (aq) + e → Ag(s) +0.80 Hg₂² (aq) + 2 e →→→ 2 Hg(l) +0.789 +0.77 +0.337 2 Hg(l) + 2 Cl(aq) +0.27 Fe³(aq) + e-→→→→→→Fe²(aq) Cu²+ (aq) + 2 e → Cu(s) HgzClz(s) + 2 e Sn¹+ (aq) + 2e → 2 H*(aq) + 2 e Pb²+ (aq) + 2 e Sn²+ (aq) +0.15 - H₂(g) 0.00 - → Pb(s) -0.126 Sn²+ (aq) + 2 e →→→Sn(s) -0.14 Ni²+ (aq) + 2 e → Ni(s) -0.25 Cd²+ (aq) + 2 e →→ Cd(s) -0.40 Cr³+ (aq) + e → Cr²+ (aq) -0.408 Fe²+ (aq) + 2 e → Fe(s) -0.44 Zn²+ (aq) + 2 e > Zn(s) -0.763 Cr²+ (aq) + 2 e →→→→Cr(s) -0.91 Al³+ (aq) + 3 e- →Al(s) -1.66 Mg²+ (aq) + 2 e →→ Mg(s) -2.37 J AG° = K=

Calculate AG and the equilibrium constant for the following reaction at 298 K: Zn²+ (aq) + Ni(s) → Zn(s) + Ni²+ (aq) Acidic Solution Standard Electrode Potential, E (volts) 2 H₂O(l) +1.77 H₂O₂(aq) + 2 H*(aq) + 2 e Au*(aq) + e — Au(s) +1.68 Au3(aq) + 3e — Au(s) +1.50 Br₂(l) +2 e 2 Br(aq) +1.08 NO3(aq) + 4 H*(aq) + 3 e NO(g) + 2 H₂O +0.96 Ag (aq) + e → Ag(s) +0.80 Hg₂² (aq) + 2 e →→→ 2 Hg(l) +0.789 +0.77 +0.337 2 Hg(l) + 2 Cl(aq) +0.27 Fe³(aq) + e-→→→→→→Fe²(aq) Cu²+ (aq) + 2 e → Cu(s) HgzClz(s) + 2 e Sn¹+ (aq) + 2e → 2 H*(aq) + 2 e Pb²+ (aq) + 2 e Sn²+ (aq) +0.15 - H₂(g) 0.00 - → Pb(s) -0.126 Sn²+ (aq) + 2 e →→→Sn(s) -0.14 Ni²+ (aq) + 2 e → Ni(s) -0.25 Cd²+ (aq) + 2 e →→ Cd(s) -0.40 Cr³+ (aq) + e → Cr²+ (aq) -0.408 Fe²+ (aq) + 2 e → Fe(s) -0.44 Zn²+ (aq) + 2 e > Zn(s) -0.763 Cr²+ (aq) + 2 e →→→→Cr(s) -0.91 Al³+ (aq) + 3 e- →Al(s) -1.66 Mg²+ (aq) + 2 e →→ Mg(s) -2.37 J AG° = K=

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
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Calculate AG and the equilibrium constant for the following reaction at 298 K: Zn²+ (aq) + Ni(s) → Zn(s) + Ni²+ (aq) Acidic Solution Standard Electrode Potential, E (volts) 2 H₂O(l) +1.77 H₂O₂(aq) + 2 H*(aq) + 2 e Au*(aq) + e — Au(s) +1.68 Au3(aq) + 3e — Au(s) +1.50 Br₂(l) +2 e 2 Br(aq) +1.08 +0.96 NO3(aq) + 4 H*(aq) + 3 e NO(g) + 2 H₂O Ag (aq) + e → Ag(s) +0.80 Hg₂² (aq) + 2 e →→→ 2 Hg(l) +0.789 +0.77 +0.337 2 Hg(l) + 2 Cl(aq) +0.27 Fe³(aq) + e-→→→→→→Fe²(aq) Cu²+ (aq) + 2 e → Cu(s) HgzClz(s) + 2 e Sn¹+ (aq) + 2e → 2 H*(aq) + 2 e Pb²+ (aq) + 2 e Sn²+ (aq) +0.15 - H₂(g) 0.00 - → Pb(s) -0.126 Sn²+ (aq) + 2 e →→→Sn(s) -0.14 Ni²+ (aq) + 2 e → Ni(s) -0.25 Cd²+ (aq) + 2 e →→ Cd(s) -0.40 Cr³+ (aq) + e → Cr²+ (aq) -0.408 Fe²+ (aq) + 2 e → Fe(s) -0.44 Zn²+ (aq) + 2 e > Zn(s) -0.763 Cr²+ (aq) + 2 e →→→→Cr(s) -0.91 Al³+ (aq) + 3 e- →Al(s) -1.66 Mg²+ (aq) + 2 e →→ Mg(s) -2.37 J AG° = K=
Transcribed Image Text:Calculate AG and the equilibrium constant for the following reaction at 298 K: Zn²+ (aq) + Ni(s) → Zn(s) + Ni²+ (aq) Acidic Solution Standard Electrode Potential, E (volts) 2 H₂O(l) +1.77 H₂O₂(aq) + 2 H*(aq) + 2 e Au*(aq) + e — Au(s) +1.68 Au3(aq) + 3e — Au(s) +1.50 Br₂(l) +2 e 2 Br(aq) +1.08 +0.96 NO3(aq) + 4 H*(aq) + 3 e NO(g) + 2 H₂O Ag (aq) + e → Ag(s) +0.80 Hg₂² (aq) + 2 e →→→ 2 Hg(l) +0.789 +0.77 +0.337 2 Hg(l) + 2 Cl(aq) +0.27 Fe³(aq) + e-→→→→→→Fe²(aq) Cu²+ (aq) + 2 e → Cu(s) HgzClz(s) + 2 e Sn¹+ (aq) + 2e → 2 H*(aq) + 2 e Pb²+ (aq) + 2 e Sn²+ (aq) +0.15 - H₂(g) 0.00 - → Pb(s) -0.126 Sn²+ (aq) + 2 e →→→Sn(s) -0.14 Ni²+ (aq) + 2 e → Ni(s) -0.25 Cd²+ (aq) + 2 e →→ Cd(s) -0.40 Cr³+ (aq) + e → Cr²+ (aq) -0.408 Fe²+ (aq) + 2 e → Fe(s) -0.44 Zn²+ (aq) + 2 e > Zn(s) -0.763 Cr²+ (aq) + 2 e →→→→Cr(s) -0.91 Al³+ (aq) + 3 e- →Al(s) -1.66 Mg²+ (aq) + 2 e →→ Mg(s) -2.37 J AG° = K=
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