Provide a cell notation for the diagram below: a. b. C. d. Copper Sulfate Solution Zn | Zn²+ || Cu²+ | Cu Cu | Cu(SO4)2 || Zn(SO4)2 | Zn Cu | Cu²+ || Zn²+ | Zn Zn | Zn(SO4)2 || Cu(SO4)2 | Cu Voltmeter salt bridge VERTEREINDER Electroc Zinc Zinc Sulfate Solution

Provide a cell notation for the diagram below: a. b. C. d. Copper Sulfate Solution Zn | Zn²+ || Cu²+ | Cu Cu | Cu(SO4)2 || Zn(SO4)2 | Zn Cu | Cu²+ || Zn²+ | Zn Zn | Zn(SO4)2 || Cu(SO4)2 | Cu Voltmeter salt bridge VERTEREINDER Electroc Zinc Zinc Sulfate Solution

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 120AE

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Question

24 Provide a cell notation for the diagram below:
a.
b.
c.
d.
Copper Sulfate
Solution
Zn | Zn²+ || Cu²+ | Cu
Cu | Cu(SO4)2 || Zn(SO4)2 | Zn
Cu | Cu²+ || Zn²+ | Zn
Zn | Zn(SO4)2 || Cu(SO4)2 | Cu
Voltmeter
salt bridge
Zinc Electroc
TESTENS
Zinc Sulfate
Solution
M

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An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
For the cell: Cr|Cr3+Co2+|Co E° is 0.46 V. The same cell was prepared in the laboratory at standard conditions. The voltage obtained was 0.40 V. A possible explanation for the difference is (a) the surface area of the chromium electrode was smaller than the cobalt electrode. (b) the mass of the chromium electrode was larger than the mass of the cobalt electrode. (c) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (d) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (e) the volume of Cr(NO3)2 solution used was larger than the volume of Cr(NO3)2 solution used.
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