3. Consider the following galvanic cell: Fe(s) Cr(s) Salt bridge containing KNO,(aq) 1M Fe+ IM Cr+ e. What happens to the mass of the Fe electrode as the redox reaction progresses? f. What happens the concentration of The Fe3+ ion as the reaction progresses? g. Which chamber will the nitrate ion flow into? (anode or cathode)

3. Consider the following galvanic cell: Fe(s) Cr(s) Salt bridge containing KNO,(aq) 1M Fe+ IM Cr+ e. What happens to the mass of the Fe electrode as the redox reaction progresses? f. What happens the concentration of The Fe3+ ion as the reaction progresses? g. Which chamber will the nitrate ion flow into? (anode or cathode)

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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Window Help 5% C Su A cvg.cengagenow.com ontent GRLContent Netflix Favorites My Home My Home My Home Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Fe"(aq) + H2(g) Fe(s) + 2H (aq) Answer: kJ K for this reaction would be than one. 團

6. When an aqueous solution of NaCl is electrolyzed, Na(l) is produced at the cathode, and Cl₂(g) is evolved at the anode. a. True b. False
2. Identify the complete redox reaction for a Zn/Zn2+||Fe³+ Fe cell. 4 A. 3 Zn (s) + 2 Fe(s) 3 Zn2+ B. 3 Zn² (aq) + 2 Fe (s) (aq) + 2 Fe³+ (aq) 3 Zn (s) + 2 Fe³ (aq) ( C. Zn (s) + 3 Fe³+ (aq) →→→ Zn²+ (aq) + 3Fe (s) D. 3 Zn (s) +2 Fe³+ (aq) →→→→3 Zn² (aq) + 2 Fe(s) 3. Identify the complete redox reaction for a Zn Zn²+AgAg cell. A. Zn(s) + Ag(s) > Zn²¹ (aq) + Ag¹ (aq) B. Zu²¹ (aq) + Ag(s) →→→ Zn (s) + Ag' (aq) C. Zn(s) + 2 Ag (aq) Zn²¹ (aq) + 2 Ag (s) >
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
A galvanic cell consist of Mg anode in a 1.0 M Mg(NO3)2 and Al cathode in a 1.0 M Al(NO3)3 solution with NaCl as the electrolyte in the salt solution. a. calculate the electrical energy b. free energy change (G) c. Equilibrium constant (K)
1.Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of the following reactions occur spontaneously. A. Zn + Ni2* → Zn2* + Ni B. 2AI + 3CI2 → 2AICI3 С. Н2 + 2Ag* → 2H* +2Ag D. 2H* + Pb → H2 Pb2+ + 2. Write the half reactions occurring at the cathode and at the anode when each cell shown in problem #1 is delivering current. 3. Calculate the voltage of the cell shown in problem #1.
54. Determine whether or not each redox reaction occurs sponta- neously in the forward direction.A. Sn2+(aq) + Zn(s) ¡ Sn(s) + Zn2+(aq)B. Mn2+(aq) + Zn(s) ¡ Mn(s) + Zn2+(aq) C. Sn2+(aq) + Pb(s) ¡ Sn(s) + Pb2+(aq) D. Au3+(aq) + Al(s) ¡ Au(s) + Al3+(aq)
a. Write the overall cell reaction/cell representation b. Calculate the stan dard cell potential (E°) c. Determine whether the reaction is spontaneous or non-spontaneous. 1. Zne) + Nia) - Zn?a) + Nie)
3. How many faradays are transferred in an electrolytic cell when a current of 2.0 amperes flows for 12 hours? a. 24 F b. 6.2 x 10-³F c. 1.1 F d. 8.6 x 104 F e. 0.90 F
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?
10. Balance the following redox reaction in acidic solution. BiO, Re- Bi- ReO,
A galvanic (voltaic) cell is made using the 2 half cells: Zn2+ (aq) + 2e → Zn(s) E =-.763 V Mg2+ (aq) + 2e - → Mg(s) with Zn(s) and Mg(s) as the electrodes. Answer the questions A. It is the anode. [Select ] B. It is the cathode. [Select] C. Electrons in the wire flow toward it. [Select]. D. Anions from the salt bridge flow toward it. [Select] E. Gains mass. [Select] E = -2.37 V F. Losses mass. [Select]