A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) || Fe2*(aq), Fe* (aq)|Pt(s) B) What is the standard potential of this cell? 1)

A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) || Fe2(aq), Fe (aq)|Pt(s) B) What is the standard potential of this cell? 1)

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 same diagram of a galvanic cell as in previous question, where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows: Ag+(aq) + e– --> Ag(s); Eo = 0.80 V Ni2+(aq) + 2e– --> Ni(s); Eo = – 0.23 V What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M. (A) 1.15 V (B) 1.30 V (C) 0.76 V (D) 0.91 V
Which of the following cell reactions would require the use of an inert electrode? O a) Zn(s) + 2Ag*(aq) → Zn²*(aq) + 2Ag(s) b) Cu(s) + 2Ag*(aq) → 2Ag(s) + Cu²*(aq) C) 3Zn2*(aq) + 2Al(s) → 3Zn(s) + 2A1³¯(aq) O d) 3Fe(s) + 2AU³*(aq) → 3FE2* + 2Au(s) e) Ni(s) + 2MnO2(s) + 2NH, (aq) → Ni²"(ag) + Mn2O3(s) + 2NH3(aq) + H2O(1)
Consider the following table of standard electrode potentials Standard Electrode Potentials at 25 °C Reduction Half-Reaction E" (V) Au" (ag) + Зе Ag"(aq) + Fe* (aq) + 3e Sn²(aq) v*(aq) + 3e In"(ag) + 3e Eu" (ag) + 3e Cr* (aq) Тa" (ag) + Зе Zn*(aq) Nb* (aq) » Au(s) 1.50 e Ag(s) 0.80 » Fe(s) -0.04 + 2e » Sn(s) -0.14 » V(s) -0.26 » In(s) -0.34 » Eu(s) -0.35 + 3e » Cr(s) -0.42 » Ta(s) -0.60 » Zn(s) » Nb(s) → Ti(s) → Al(s) » Be(s) + 2e -0.76 + 3e -1.10 Ti (aq) + 2e Al" (aq) + 3e Ве (ag) + 2е Am* (ag) + 2e -1.63 -1.66 -1.85 » Am(s) -1.90 Pr* (ag) + 2e" » Pr(s) -2.00 Mg* (aq) + 20 - Mg(s) » Na(s) » Ca(s) -2.37 Na (aq) + Ca*(aq) Sr* (aq) + 2e Ba (aq) e -2.71 2e - 2.87 » Sr(s) -2.90 + 2e + Ba(s) -2.91
30) Write the balanced overall reaction and calculate the standard cell emf (E) for: Al(s) | Al"(aq) || I, (s) | I(aq) | Pt(s)
Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq) (a) (b) (c) O Strength of oxidizing agent cell V not spontaneous spontaneous Selected Standard Electrode Potentials (298 K) Half-Reaction F2(g) + 2e7 Cl₂(g) + 2e7 MnO₂(s) + 4H+ (aq) + 2e7 NO3(aq) + 4H+ (aq) + 3e¯ Ag+ (aq) + e Fe³+ (aq) + e O₂(g) + 2H₂O() + 4e Cu²+ (aq) + 2e7 2H+ (aq) + 2e7 N₂(g) + 5H+ (aq) + 4e¯ Fe2+ (aq) + 2e7 2+ Zn²+ (aq) + 2e 2H₂O() +2e7 Na+ (aq) + e 2F (aq) 2C1 (aq) 2+ Mn²+ (aq) + 2H₂O(l) NO(g) + 2H₂O(l) Ag(s) Fe²+ (aq) 4OH(aq) Cu(s) H₂(g) N₂Hs+ (aq) Fe(s) Zn(s) H₂(g) + 2OH(aq) Na(s) Strength of reducing agent E half-cell (V) +2.87 +1.36 +1.23 +0.96 +0.80 +0.77 +0.40 +0.34 0.00 -0.23 -0.44 -0.76 -0.83 -2.71
2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)
Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
The potential of the following voltaic cell is 0.55 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell.
6. The above diagram shows a Galvanic constructed from Ag|AGNO3(aq) and Ni|Ni(NO3)2(aq) half-cells and the half-cell electrode potentials are as follows: Ag*(aq) + e--> Ag(s); E° = 0.80 V %3! Ni2*(aq) + 2e --> Ni(s); E° = - 0.23 V Calculate the Ecell at 25°C when the electrolyte concentrations are: [Ag*] = 1.3 x %3D 10-4 M and [Ni2+] = 0.10 M. %3D
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
For the cell shown, the measured cell potential E cell -0.365; V at 25 degrees * C . Pr(s)|H 2 (g,0.803 am)|H^ + (aq,?M)||Cd^ 2+ (aq,1.00 M)|Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values E ^ o are 2H^ + (aq)+2e^ - longrightarrow H 2 (g) E ^ o = 0.00V Cd^ 2+ (aq)+2e^ - longrightarrow Cd(s) E ^ o= - 0.403V Calculate the H^ + concentration.
The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s) | ZnO(s) | KOH(aq) || Ag2O(s) | Ag(s) (+) Write the balanced equation for the net cell reaction equation