11. Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • a Cu electrode in 1.0 M CuCl, solution • a Ni electrode in 1.0 M Ni(NO3 )2 solution a. WHICH ELECTRODE LOSES MASS? • a Mg electrode in 1.0 M MgCl, solution • a Fe electrode in 1.0 M FeCl, solution b

11. Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. • a Cu electrode in 1.0 M CuCl, solution • a Ni electrode in 1.0 M Ni(NO3 )2 solution a. WHICH ELECTRODE LOSES MASS? • a Mg electrode in 1.0 M MgCl, solution • a Fe electrode in 1.0 M FeCl, solution b

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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Calculate Ecel (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.793 M and the concentration of the ion at the cathode is 1.90 M. Use the standard reduction potentials from Appendix L in our textbook. Np + Lu³* » Lu + Np3*
3. Calculate the free energy, AG°, for each electrochemical cell given the following information and determine if the reaction is spontaneous or nonspontaneous. T= 298 K a. E cell =+ 2.10 V, n= 2 b. Каg— 2.2 х 10-3 c. E cell =- 0.677 V, n = 3 =
78. A voltaic cell consists of a Pb/Pb2 half-cell and a Cu/Cu2" half- cell at 25 C. The initial concentrations of Pb and Cu are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential? b. What is the cell potential when the concentration of Cu2" has fallen to 0.200 M? c. What are the concentrations of Pb- and Cu" when the cell potential falls to 0.35 V?
3. Consider the following half-cell reactions and associated standard half-cell potentials Ag* + e -> Ag Cu2 + 2e -> Cu Ni2 + 2e -> Ni Cr3 + 3e -> Cr a. Write the overall reaction using the list above that leads to the maximum positive standard potential. b. What is the maximum standard potential?
6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.
A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
Set up a cell that has a Mg electrode in a 1.0 M aqueous Mg²+ solution on the left side and a Cu electrode in a 1.0 M aqueous Cu2+ solution on the right side. Add the salt bridge. What is the anode of this system? the Cu electrode the Mg electrode What is the cathode of this system? the Cu electrode O the Mg electrode
11. The following two half-cells are connected to form a full Galvanic cell: Cu"(aq) +2e Au (aq) +e → Cu(s) → Au(s) E° = 0.34 V E 1.69 V a. Calculate E° for the cell. b. Give the cell notation for this system. c. Give the balanced cell reaction. d. Calculate AG for the reaction e. Calculate Keg for the reaction. £. Calculate the cell potential if the activity of Cu is 0.0100 and the activity of Au" is 1.340.
4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…
Set up a cell that has a Mg electrode in a 1.0 M aqueous Mg2+ solution on the left side and a Cu electrode in a 1.0 M aqueous Cu2+ solution on the right side. Add the salt bridge. What is the balanced net ionic equation for this reaction? Include physical states.