80. Consider the concentration cell:Pb(s)Salt bridgecontainingNaNO3(aq)2.5 M Pb2+5.0 × 10 ³M Pb2+a. Label the anode and cathode.Pb(s)b. Indicate the direction of electron flow.c. Indicate what happens to the concentration of Pb2+ in eachhalf-cell.

Anode is where oxidation occurs, and cathode is where reduction occurs. Oxidation is the process of…

Answered: 80. Consider the concentration cell:…

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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For the following voltaic cell:Fe(s) | Fe^2+(aq, 1.0 M) || Cu^2+(aq, 1.00 M) | Cu(s) a. Draw a diagram of the cell.b. Write the cell half-reactions.c. Label one half-reaction as the oxidation, the other as the reduction.
6. Consider a galvanic cell consisting of an Al electrode placed in a 1 M Al(NO3)3 solution and a Ag electrode placed in a 1 M AgNO3 solution. a.)Write the half-reaction which occurs at the anode. b.)Write the half-reaction which occurs at the cathode c.)Write a balanced net ionic equation for the galvanic cell. d.)Calculate the standard emf of the cell e.)Give the cell diagram for the reaction occurring in this galvanic cell. f.)What is oxidized? g.)What is the oxidizing agent?
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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?
An electrochemical cell has a positive standard cell potential but a negative cell potential. Which statement is true? a. K> 1; Q > K b. K K c. K> 1; Q < K d. K< 1; Q< K
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. Sketch the apparatus that could be used to study the following reaction. Label anode, cathode, and solutions in each half cell in your sketch. Ti (s) + Cd2+ (aq) → Ti²+ (aq) + Cd (s) b. Use the A |A* || B+ | B expression to represent the cell you have drawn in (a)
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.
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…
10. A galvanic cell was set up using zinc and tin. The set up is shown below. Zn Sn Salt Bridge 1.0 M Sn²+ 1.0 M Zn²+ Choose 2 of the following statements to explain. Be sure to include balanced equations as part of your response. a. Using the reduction potential table, predict the cell voltage for this cell. b. What is the reaction at the cathode? c. Which electrode do you expect will lose mass? d. What is the direction of the movement of ions and the electron flow?

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80. Consider the concentration cell: Pb(s) Salt bridge containing NaNO3(aq) 2.5 M Pb2+ 5.0 × 10 ³M Pb2+ a. Label the anode and cathode. Pb(s) b. Indicate the direction of electron flow. c. Indicate what happens to the concentration of Pb2+ in each half-cell.