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19. Given Fe + 2e → Fe, o° =-0.440 v, and Fe +eFe", o° = 0.771 V, cal- culate o° for Fe* + 30 Fe 20. Given O, + 2H,0 + 4e → 40H, 0° = 0.401 V, calculate o° for O, + 4H + 4e → 2H,O. 21. Calculate the pressure (fugacity) of hydrogen required to stop corrosion of iron immersed in 0.1 M FeCl, pH = 3.

19. Given Fe + 2e → Fe, o° =-0.440 v, and Fe +eFe", o° = 0.771 V, cal- culate o° for Fe* + 30 Fe 20. Given O, + 2H,0 + 4e → 40H, 0° = 0.401 V, calculate o° for O, + 4H + 4e → 2H,O. 21. Calculate the pressure (fugacity) of hydrogen required to stop corrosion of iron immersed in 0.1 M FeCl, pH = 3.

Chemistry
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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18. Calculate the emf as in Problem 17 in an air-saturated alkaline solution of pH = 10. Which electrode corrodes on short-circuiting the cell? (Assume that HP6O; forms as corrosion product and that its activity is 0.1; also assume that iron is passive and that its potential approximates the oxygen electrode.) HP6O, +H,O+ 2e → Pb+ 30H °=-0.54V 19. Given Fe* + 2e → Fe, o° =-0.440 v, and Fe* +e → Fe", o° = 0.771 V, cal- culate o° for Fe* + 3e Fe 20. Given O, + 2H,O + 4e → 40H , o° = 0.401 V, calculate o for O, + 4H + 4e → 2H,O. 21. Calculate the pressure (fugacity) of hydrogen required to stop corrosion of iron immersed in 0.1 M FeClz, pH = 3. 22. Calculate the pressure of hydrogen, as in Problem 21, in deaerated water with Fe(OH), as the corrosion product. [Solubility product Fe(OH), = 1.8 x 23. Calculate the pressure of hydrogen required to stop corrosion of cadmium at 25 °Cin deaerated water, with Cd(OH); as the corrosion product. [Solubil- ity product Cd(OH). = 2.0 x 10-41 24. A copper storage tank containing dilute H,SO, at pH = 0.1 is blanketed with hydrogen at latm. Calculate the maximum Cu contamination of the acid in moles Cu per liter. What is the corresponding contamination if the hydro- gen partial pressure is reduced to 10 atm?
Transcribed Image Text:18. Calculate the emf as in Problem 17 in an air-saturated alkaline solution of pH = 10. Which electrode corrodes on short-circuiting the cell? (Assume that HP6O; forms as corrosion product and that its activity is 0.1; also assume that iron is passive and that its potential approximates the oxygen electrode.) HP6O, +H,O+ 2e → Pb+ 30H °=-0.54V 19. Given Fe* + 2e → Fe, o° =-0.440 v, and Fe* +e → Fe", o° = 0.771 V, cal- culate o° for Fe* + 3e Fe 20. Given O, + 2H,O + 4e → 40H , o° = 0.401 V, calculate o for O, + 4H + 4e → 2H,O. 21. Calculate the pressure (fugacity) of hydrogen required to stop corrosion of iron immersed in 0.1 M FeClz, pH = 3. 22. Calculate the pressure of hydrogen, as in Problem 21, in deaerated water with Fe(OH), as the corrosion product. [Solubility product Fe(OH), = 1.8 x 23. Calculate the pressure of hydrogen required to stop corrosion of cadmium at 25 °Cin deaerated water, with Cd(OH); as the corrosion product. [Solubil- ity product Cd(OH). = 2.0 x 10-41 24. A copper storage tank containing dilute H,SO, at pH = 0.1 is blanketed with hydrogen at latm. Calculate the maximum Cu contamination of the acid in moles Cu per liter. What is the corresponding contamination if the hydro- gen partial pressure is reduced to 10 atm?
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