1. Predict whether the following reactions arespontaneous: [assume SHE value is zero]a) Pd (aq)?+ + H, (g) -à Pd (s) + 2H† (aq)b) Sn (aq)++ + H, (g) -à Sn(aq)2+ + 2H* (aq)c) Ni (aq)?* + H, (g) -à Ni (s) + 2H* (aq)d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq)Given Pd+/Pd =0.987 V, Snª*/ Sn²+ =0.154 V,Ni²*/Ni = -0.250 V, Cď*/Cd = -0.403 VFrom your answers, decide which of the abovemetals/metal ion could be reduced by hydrogen.2. Identify the oxidizing agents and reducing agents inthe above reaction (1.)3. Using the standard potentials, Calculate Eand equilibrium constant for the followingtwo reactions:→ 2 TI(s) + Cl,(g)a) TI*(aq) + 2 C(aq)given the following standard reduction potentials.Cl,(g) + 2 e →TI*(aq) + e →E° = +1.36 V2 Cl(aq)TI(s)E° = -0.34 V5 Cd2+b) 5 Cd(s) + 2 MnO,¯(aq) + 16 H*(aq)(aq) + 2 Mn²*(aq) + 8 H,O(1); given thefollowing standard reduction potentials.MnO4 (aq) + 8 H*(aq) + 5 e → Mn²*(aq) + 4H,O1)Сd+(aq) + 2 е —>E° = +1.52 VCd(s)E° = -0.40 V

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spontaneous: [assume SHE value is zero] a) Pd (aq)2+ + H, (g) -à Pd (s) + 2H* (aq) b) Sn (aq)++ + H, (g) -à Sn(aq)2++ 2H* (aq) c) Ni (aq)2+ + H, (g) -à Ni (s) + 2H* (aq) d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq) Given Pd*/Pd =0.987 V, Snª*/ Sn²+ =0.154 V, Ni²+/Ni = -0.250 V, Cď*/Cd = -0.403 V From your answers, decide which of the above

spontaneous: [assume SHE value is zero] a) Pd (aq)2+ + H, (g) -à Pd (s) + 2H* (aq) b) Sn (aq)++ + H, (g) -à Sn(aq)2++ 2H* (aq) c) Ni (aq)2+ + H, (g) -à Ni (s) + 2H* (aq) d) Cd (aq)²+ + H, (g) -à Cd (s) + 2H* (aq) Given Pd/Pd =0.987 V, Snª/ Sn²+ =0.154 V, Ni²+/Ni = -0.250 V, Cď*/Cd = -0.403 V From your answers, decide which of the above

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 10ALQ

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