Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Question
Chapter 1, Problem 1.78E
Interpretation Introduction
Interpretation:
Table 1.4 gives different values of the second virial coefficient B for different temperatures. Assuming standard pressure of 1 bar, the molar volumes of He, Ne, and Ar for the different temperatures is to be determined. A graph of V versus T is to be determined.
Concept introduction:
In reality, the gases we encounter deviate from the ideal gas equations at low temperature and high pressure. These gases are non-ideal gases or real gases. Moreover, the behavior of non-ideal gases can be best explained by state equations, but they are quite complicated. Generally, for one mole of an ideal gas the equation can be written as pῡ/RT = 1.
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Chapter 1 Solutions
Physical Chemistry
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- Use the ideal gas law to symbolically prove the cyclic rule of partial derivatives.arrow_forwardThe ideal gas law is theequation of state for an ideal gas. Why cantit be used to determine TpH?arrow_forwardUnder what conditions would the van der Waals constant b be negative? Do you think there are any gases for which this occurs?arrow_forward
- Why is nitrogen a good choice for the study of ideal gas behavior around room temperature?arrow_forwardUnder what conditions of temperature does a Redlich-Kwong gas behave like an ideal gas? Use the Redlich-Kwong equation of state to justify your answer.arrow_forwardUnder what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?arrow_forward
- Referring to exercises 1.6 and 1.7, does it matter if the pressure difference is caused by an ideal gas or a non-ideal gas? Explain your answer.arrow_forwardWhat properties of a nonideal gas do the Vander Waals constants represent?arrow_forwardTable 1.4 show that the second virial coefficient B for He is negative at low temperature, seems to maximize at a little over 12.0 cm3/mol, and then decreases. Do you think it will become negative again at higher temperatures? Why is it decreasing?arrow_forward
- Use the approximation 1 x-1 1 x x2 to determine an expression for the virial coefficient C in terms of the van der Waals constants.arrow_forwardAt the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forwardPerform a units analysis on the exponent of the barometric function and verify that the overall exponent is unitless.arrow_forward
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