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Ch.10 - Gases
All textbooksBrown 14th EditionCh.10 - GasesProblem 113g
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Chapter 10, Problem 113g

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (g) Which one would have the largest van der Waals b parameter?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Van der Waals Forces

Van der Waals forces are weak intermolecular forces that arise from temporary dipoles in molecules. These forces include attractions between neutral molecules and are significant in understanding the behavior of gases and liquids. The strength of these forces can influence properties such as boiling points and solubility.
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Van der Waals Equation

Van der Waals b Parameter

The Van der Waals b parameter represents the volume occupied by one mole of a gas at a given temperature and pressure, accounting for the finite size of gas molecules. A larger b value indicates that the molecules are larger or more complex, leading to greater repulsive interactions. This parameter is crucial for understanding deviations from ideal gas behavior.
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STP Conditions

Standard Temperature and Pressure (STP) refers to a set of conditions commonly used in chemistry, defined as 0 degrees Celsius (273.15 K) and 1 atmosphere of pressure. Under these conditions, the behavior of gases can be compared more easily, and properties such as molar volume can be standardized, aiding in the analysis of different gases.
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STP Calculation Example
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Related Practice
Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (a) Which gas is most likely to depart from the assumption of the kinetic-molecular theory that says there are no attractive or repulsive forces between molecules?

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Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (d) Which one has the highest total molecular volume relative to the space occupied by the gas?

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Textbook Question

Consider the following gases, all at STP: Ne, SF6, N2, CH4. (f) Which one would effuse more rapidly than N2?

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Textbook Question
It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms (b) at 20.27 MPa pressure and 0 °C. (Assume for simplicity that the ideal-gas equation still holds.)
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Textbook Question

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose 120.00 kg of N21g2 is stored in a 1100.0-L metal cylinder at 280 °C. (b) By using the data in Table 10.3, calculate the pressure of the gas according to the van der Waals equation.

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Textbook Question

Cyclopropane, a gas used with oxygen as a general anesthetic, is composed of 85.7% C and 14.3% H by mass. (a) If 1.56 g of cyclopropane has a volume of 1.00 L at 99.7 kPa and 50.0 °C, what is the molecular formula of cyclopropane?

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