49. The following diagram shows a Ammeter molecular view of the electrochemical cell diagrammed in Figure 14.2. Draw a molecular view showing the changes that occur after the cell has produced electrical current for some extended Zn(s)- anode - Cu(s) cathode Salt bridge period of time. Zn2+ Cu2+ Zn(NO3)2(aq) `Cu(NO3)2(aq) Oxidation Reduction

49. The following diagram shows a Ammeter molecular view of the electrochemical cell diagrammed in Figure 14.2. Draw a molecular view showing the changes that occur after the cell has produced electrical current for some extended Zn(s)- anode - Cu(s) cathode Salt bridge period of time. Zn2+ Cu2+ Zn(NO3)2(aq) `Cu(NO3)2(aq) Oxidation Reduction

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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Use the standard reduction potentials given below to predict if a reaction will occur between Ag(s) and F2 (g), when the two are brought in contact via standard half-cells in a voltaic cell. F2 (g)+2e7 →2F (aq) E red Agt (ag)+e → Ag(s) E red + = If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - 2.870 V 0.799 V +
2. In a galvanic cell, Cr(s) oxidizes to form Cr³+ (aq) while Cu²+ (aq) reduces to form Cu(s). Write its cell notation (line notation).
Which of the following metals can be oxidized by H+ under standard conditions? Cu, Zn, Ag, Sn Ag+(aq) + e– → Ag(s) E° = 0.80 V Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Cu2+(aq) + e– → Cu+(aq) E° = 0.15 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V Sn2+(aq) + 2e– → Sn(s) E° = –0.14 V Zn2+(aq) + 2e– → Zn(s) E° = –0.76 V
13. Write the oxidation half reaction, the reduction half reaction, and the overall cell reaction for the following galvanic cell. Identify the anode and the cathode and state why you labeled the metals that way. (4) Zn (s) | Zn²+ (aq) || Cu²+ (aq) | Cu (s)
Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Ni Ag 1.0 M Ni2+ 1.0 M Ag* The standard reduction potentials are as follow: Ni2+ + 2 e- → Ni(s), E° = -0.25 Ag* + e - Ag(s), E° = 0.7996 When current is allowed to flow, which species is oxidised? Select one: а. Ag b. Cannot be determined from the data given. C. Ni2+ O d. Ag* O e. Ni
A galvanic cell was formed using Avium and Beanium:[hypothetical elements] Reduction Potentials: Av3+(aq) + 3e- → Av(s) Eo = -0.48 V Bn4+(aq) + 4e- → Bn(s) Eo = +0.15 V a) Write a net ionic equation for this reaction. b) Write the cell notation for this cell. c) Which is the oxidizing agent? Explain how you know.
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)
What reactions take place at the cathode and the anode when each of the following solutions is used in an electrolytic cell? Write the half-reaction equations for the anode and cathode, and state whether the reaction would result in metal being plated onto the object. 1.0 mol/L aluminum fluoride solution, AlF3(aq)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction + 21O3(aq)+ 12 H¹ (aq)+10e¯ Cl₂(g) +2e 1₂(s) + 6H₂O(1) → 2 C1 (aq) standard reduction potential E=+1.195 V 'red E 70 = +1.359 V red
Consider the following half reactions: M²+ (aq) + 2e (aq) → M(S) X³+ (aq) + 3e (aq) →→→→→→X(s) Eº=-0.4 Eº=-0.7 Calculate the overall cell potential for the overall spontaneous redox reaction. Give your answer to one decimal place.
A particular voltaic cell operates on the reaction below, giving an emf of 0.853 V. Calculate the maximum electrical work (in kJ) generated when 20.2 g of zinc metal is consumed. Zn(s) + CI2(g) → Zn2+(aq) + 2 Cl −(aq)