For the following reaction show on the diagram above. Fe(s) + Cu2*(ag) →> Fe2*(ag) + Cu(s) 1. Electron flow 2. Salt bridge 3. Anode 4. Cathode 5. Put sign-plus or negative on each electrode 6. Cation flow 7. Anion flow 8. Calculate E° for the cell. Show your work. 9. Is the reaction spontaneous as it is written? 10. If the concentration of the iron ion is 0.10 M and the concentration of the Cu ion is 0.10 M, what is the E of the cell? Show your work.

For the following reaction show on the diagram above. Fe(s) + Cu2(ag) →> Fe2(ag) + Cu(s) 1. Electron flow 2. Salt bridge 3. Anode 4. Cathode 5. Put sign-plus or negative on each electrode 6. Cation flow 7. Anion flow 8. Calculate E° for the cell. Show your work. 9. Is the reaction spontaneous as it is written? 10. If the concentration of the iron ion is 0.10 M and the concentration of the Cu ion is 0.10 M, what is the E of the cell? Show your work.

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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An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode Based on the reactions below, which is the stongest reducing agent? +1.22 V MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2- (aq) -0.95 V SnO2(s) + 2H2O() + 4e-→ Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- → Cr(s) + 3OH-(aq) a.Hg2SO4 b.Mn02 c.Cr d.Sn e.Hg Identify the strongest oxidizing agent from the following half-reactions. The standard reduction potentials are listed. +1.22 V Mn02(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H20(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2-(aq) -0.95 V SnO2 (s) + 2H2O() + 4e- Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- Cr(s) + 3OH- (aq) a. MnO2 b.Hg2SO4 c.Sn d.Hg e.Cr
k Please don't provide handwritten solution
15. Which of the following determines if a redox reaction is spontaneous? a. a positive cell potential b. a negative cell potential c. the reducing agent on the left is stronger than the reducing agent on the right d. two of the above are correct 16. What is the correct standard cell notation for a zinc-copper cell? a. Cu²+ (aq) | Cu(s) || Zn(s) | Zn²+ (aq) c. Cu(s)| Cu²+ (aq) || Zn²+ (aq) Zn(s) 7 b. Cu(s) Cu²+ (aq) || Zn(s)| Zn²+ (aq) d. Zn(s) Zn²+ (aq)| Cu²+ (aq) | Cu(s)
For each set of electrodes, fill in the table below. Write the balanced reaction that occurs. You will have each balanced reaction listed more than once. If the anodes are connected correctly to measure the spontaneous reaction, write “Y, otherwise write “N” in the “Spontaneous” column. Black Lead .001 Cu (NO3)2 Red Lead .01 M Cu (NO3)2 Voltage .0175 Spontaneous is Yes for this one I need the balance equation for the above. Black Lead Red Lead Ecell (obs) Balanced equation Spontaneous Cu(0.001) Cu(0.01)
12. Electrochemistry is important in many aspects of daily life. i. Define voltaic cell. ii. Fill in the blanks for the drawing of a voltaic cell that's made with copper/copper (II) nitrate (E° = 0.34 V) and zinc/zinc (II) nitrate (E° = -0.76 V). Briefly explain the role of the salt bridge. iii. Using the equation Eᵒcell = E° cathode E anode, calculate the overall cell potential for the cell in step b. Be sure to show all steps completed to arrive at the answer. h. a. b. C. d. e. 1845 f. g. h. b. C. 9- C. d. h
For each of the electrolyte electrode pairings, indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables. Write the conventional cell notation. a. Zn and Zn² mixed with Pb and Pb+² b. Cu and Cu2 mixed with Ag and Ag*
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2. For the following concentration cell, use the Nernst equation to determine the expected voltage. Also indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables from powerpoint slides 11 and 12 and the Nernst equation. Once you have determined the cell reaction, write the conventional cell notation. Zn and Zn+2 (0.25M) mixed with Cu and Cu+2 (0.35M)
22. The diagram below represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell? Al(s))Al³*(1.0 M)||Cu²*(1.0 M)|Cu(s) a. Al(s) + Cu (ag)→ Al** (aq) + Cu(s) b. 2H,0) + 3A1*(aq) + 2Cu(s) → 2A1(s) + 3Cu?*(aq) + 4H*(aq) + 0,(g) c. 2Al(s) + 3Cu?*(aq) → 3AI** (aq) + 2Cu(s) d. Al*(aq) + Cu(s) → Al(s) + Cu?*(aq) e. 3A* (aq) + 2Cu(s) → 2Al(s) + 3Cu²*(aq)
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)
The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Al(s) + 312 (s) → 2Al3+ (aq) + 6I¯ (aq) 3+ The emf generated by the cell when [Al] = 3.0 · 10- M and [I¯] = 0.50 M is %3D V. 2.23 2.27 2.20 2.13 2.34
Consider a cell that uses the redox reaction: Cu2+ (aq) + Zn (s) → Zn2+ (aq) + Cu (s). The standard reduction potentials for the two half reactions that make up this cell are shown below. A potentiometer is used to measure the potential difference between two half cells. What is the reading on the potentiometer when [Cu2+] = 0.010 M and [Zn2+] = 0.10 M. Cathode: Cu2+(aq) + 2e- → Cu(s) E° = 0.34 V Anode: Zn2+(aq) + 2e- → Zn(s) E° = -0.76 V 1.10 V 1.04 V 1.07 V 1.13 V