[3] ~ Electrolytes Consider the following half-cells, where you are given their reduction potentials and molalities: Eºr red=+0.80 V & red=0.31 V * Ag(s) Agt (m1), NO3- (m1); * Pb(s) PbSO4(s), SO4²- (m2), K+ (2m2); where m₁ = 0.003 mol/kg and m2-0.009 mol/kg. (a) Make a scheme of a Galvanic battery that involves these half cells and show which are the anode and cathode. (Make a reasonable choice of salt bridge that reduces the liquid juncture potential AOLJ.) (b) Write the Nernst equation, using the Debye-Hückel limit law for the activity coefficients. (c) Calculate the electromotive force for the battery at 298K.

[3] ~ Electrolytes Consider the following half-cells, where you are given their reduction potentials and molalities: Eºr red=+0.80 V & red=0.31 V * Ag(s) Agt (m1), NO3- (m1); * Pb(s) PbSO4(s), SO4²- (m2), K+ (2m2); where m₁ = 0.003 mol/kg and m2-0.009 mol/kg. (a) Make a scheme of a Galvanic battery that involves these half cells and show which are the anode and cathode. (Make a reasonable choice of salt bridge that reduces the liquid juncture potential AOLJ.) (b) Write the Nernst equation, using the Debye-Hückel limit law for the activity coefficients. (c) Calculate the electromotive force for the battery at 298K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e" Co2*(aq) + 2e → Ag(s) 0.799V → Co(s) |-0.280V Zn2*(aq) + 2e → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Zn2*(aq) oxidize Ag(s) to Ag"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Consider the following cell: | Zn (s) | Ca2* (aq) , SO3²- (aq) || Hg²+ (aq) , F' (aq) | Pt (s) | al Indiate the Oxidizing Agent bindicate the ReducingAge Gont e Wnte he narreattions that occurs ai the cathode d) Write the half reactions that occurs at the anode e) Write the overall net cell reaction f) Calculate the cell potential g) Indicate if electricity is produced or consumed by the cell h) Indicate if the cell is galvanic or electrolytic
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh
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e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
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