Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 1, Problem 1.30E
Determine the expressions for the following, assuming that the
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Which on the following statements is false?
In a mixture, each gas can not be considered ideal, therefore one can not use the
ideal gas equation in order to determine the partial pressure of a particular gas.
The molar volume is the same for all ideal gases at STP.
The total pressure of a particular gas in a mixture of gases can be determined by
multiplying the total pressure of the mixture by the mole fraction (# of moles of
the gas in question divided by the total number of moles) of the gas in question.
In general, amount of vapour pressure increases with a rise in temperature.
In a mixture of gases, the total pressure is equal to the sum of the partial
pressures of each gas in the mixture.
1. Determine the expression for (), for (a) a gas following
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Tin
the van der Waals equation and (b) virial equation.
Dalton's law states that in a mixture of chemically non-interacting gases, thethe pressure exerted by each contributor at a certain temperature is the same as if it were alone in thein the container alone, and that the total pressure is equal to the sum of the partial pressures(1) of each gas. Deduce this law by kinetic theory from equation 18.11.
(1)The partial pressure of a gas in a mixture of ideal gases corresponds to the pressure it would exert if it werealone, occupying the whole container, at the same temperature of the ideal mixture.
P = F/A = N*m*Vx^2/V (18.11)
Chapter 1 Solutions
Physical Chemistry
Ch. 1 - A bomb calorimeter is a study metal vessel in...Ch. 1 - Difference between the system and the...Ch. 1 - Prob. 1.3ECh. 1 - Prob. 1.4ECh. 1 - Prob. 1.5ECh. 1 - Prob. 1.6ECh. 1 - Prob. 1.7ECh. 1 - A pot of cold water is heated on a stove, and when...Ch. 1 - hat difference is necessary for heat to flow...Ch. 1 - What is the value of FT for a sample of gas whose...
Ch. 1 - What is the value of FP for a sample of gas whose...Ch. 1 - Prob. 1.12ECh. 1 - Hydrogen gas is used in weather balloon because it...Ch. 1 - Prob. 1.14ECh. 1 - A 2.0 L soda bottle is pressurized with 4.5 atm of...Ch. 1 - The Mount Pinatubo volcano eruption in 1991...Ch. 1 - Prob. 1.17ECh. 1 - Scottish physicist W. J. M. Rankine proposed an...Ch. 1 - Use the two appropriate values of R to determine a...Ch. 1 - Prob. 1.20ECh. 1 - Pressures of gases in mixtures are referred to as...Ch. 1 - Earths atmosphere is approximately 80 N2 and 20...Ch. 1 - The atmospheric surface pressure on Venus is 90...Ch. 1 - Prob. 1.24ECh. 1 - Prob. 1.25ECh. 1 - In the anaerobic oxidation of glucose by yeast,...Ch. 1 - What are the slopes of the following lines at the...Ch. 1 - For the following function, evaluate the...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Determine the expressions for the following,...Ch. 1 - Prob. 1.31ECh. 1 - Prob. 1.32ECh. 1 - Prob. 1.33ECh. 1 - Prob. 1.34ECh. 1 - What properties of a nonideal gas do the Vander...Ch. 1 - Prob. 1.36ECh. 1 - Prob. 1.37ECh. 1 - Calculate the Boyle temperatures for carbon...Ch. 1 - Prob. 1.39ECh. 1 - Prob. 1.40ECh. 1 - Table 1.4 show that the second virial coefficient...Ch. 1 - Prob. 1.42ECh. 1 - What is the van der Waals constant a for Ne in...Ch. 1 - Prob. 1.44ECh. 1 - Under what conditions would the van der Waals...Ch. 1 - By definition, the compressibility of an ideal gas...Ch. 1 - The second virial coefficient B and the third...Ch. 1 - Use the approximation 1 x-1 1 x x2 to...Ch. 1 - Why is nitrogen a good choice for the study of...Ch. 1 - Evaluate for a gas following the Redlich-Kwong...Ch. 1 - Numerically evaluate for one mole of methane...Ch. 1 - Under what conditions of volume does a van der...Ch. 1 - At high temperatures, one of the van der Waals...Ch. 1 - Under what conditions of temperature does a...Ch. 1 - The Berthelot equation of state for one mole of...Ch. 1 - Prob. 1.56ECh. 1 - Referring to exercises 1.6 and 1.7, does it matter...Ch. 1 - Prob. 1.58ECh. 1 - Use Figure 1.11 to construct the cyclic rule...Ch. 1 - Prob. 1.60ECh. 1 - Prob. 1.61ECh. 1 - Calculate for one mole of an ideal gas at STP and...Ch. 1 - Prob. 1.63ECh. 1 - Show that = T/p for an ideal gas.Ch. 1 - Determine an expression for V/T p, n in terms of ...Ch. 1 - Prob. 1.66ECh. 1 - Prob. 1.67ECh. 1 - Perform a units analysis on the exponent of the...Ch. 1 - Using the barometric formula, calculate the...Ch. 1 - The barometric formula can also be used for...Ch. 1 - Prob. 1.71ECh. 1 - Prob. 1.72ECh. 1 - Prob. 1.73ECh. 1 - Prob. 1.74ECh. 1 - Prob. 1.75ECh. 1 - Prob. 1.76ECh. 1 - Prob. 1.77ECh. 1 - Prob. 1.78ECh. 1 - Prob. 1.79ECh. 1 - Use the ideal gas law to symbolically prove the...Ch. 1 - Prob. 1.81E
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- Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?arrow_forwardUnder what conditions of volume does a van der Waals gas behave like an ideal gas? Use the van der Waals equation of state to justify your answer.arrow_forwardPerform a units analysis on the exponent of the barometric function and verify that the overall exponent is unitless.arrow_forward
- Analogous to equation 4.26, what is the expression for U, assuming one knows the behavior of A as it varies with respect to temperature and volume?arrow_forwardAt what temperature (C) will 0.810mol of chlorine in a 15.7L vessel exert a pressure of 756torr?arrow_forwardperform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.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_forwardWhy is nitrogen a good choice for the study of ideal gas behavior around room temperature?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
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