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1. Calculate the value for 2.303 RT/F at 50°C.

1. Calculate the value for 2.303 RT/F at 50°C.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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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 half-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 H2 = 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 deacer- 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-.
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 half-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 H2 = 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 deacer- 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-.
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