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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![PROBLEMS
In these problems, temperature is 25 °C unless otherwise stated.
1. Calculate the value for 2.303 RT/F at 50°C.
2. Calculate the exact hall-cell potential for the Ag-AgCI electrode in 1M
NaCl.
3. Calculate the exact half-cell potential of zinc in 0.01 M ZnCl.
4. Calculate the half-cell potential of the hydrogen electrode in a solution of
pH = 7 and partial pressure of H. = 0.5 atm at 40°C.
5. The emf of a cell made up of zinc (anode) and hydrogen electrode (cathode)
immersed in 0.5 M ZnCl, is +0.590 V. What is the pH of the solution?
6. Calculate the theoretical tendency of zinc to corrode (in volts) with evolution
of hydrogen when immersed in 0.01 M ZnCl, acidified to pH = 2
7. Calculate the theoretical tendency for nickel to corrode (in volts) in deaer-
ated water of pH=7. Assume that the corrosion products are H, and Ni(OH),,
the solubility product of which is 1.6 x 10-1,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F593b8f9b-950b-48cb-bb79-7a7be003cf58%2Fd2e3ea8b-d1fd-46ee-88b6-b1025a4a3b46%2F0send5b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:PROBLEMS
In these problems, temperature is 25 °C unless otherwise stated.
1. Calculate the value for 2.303 RT/F at 50°C.
2. Calculate the exact hall-cell potential for the Ag-AgCI electrode in 1M
NaCl.
3. Calculate the exact half-cell potential of zinc in 0.01 M ZnCl.
4. Calculate the half-cell potential of the hydrogen electrode in a solution of
pH = 7 and partial pressure of H. = 0.5 atm at 40°C.
5. The emf of a cell made up of zinc (anode) and hydrogen electrode (cathode)
immersed in 0.5 M ZnCl, is +0.590 V. What is the pH of the solution?
6. Calculate the theoretical tendency of zinc to corrode (in volts) with evolution
of hydrogen when immersed in 0.01 M ZnCl, acidified to pH = 2
7. Calculate the theoretical tendency for nickel to corrode (in volts) in deaer-
ated water of pH=7. Assume that the corrosion products are H, and Ni(OH),,
the solubility product of which is 1.6 x 10-1,
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