A scientist uses extreme temperature environments to study the non-ideal behavior of gas molecules. One way to increase the non-ideal behavior of gas molecules under investigation would be to:

Question

A scientist uses extreme temperature environments to study the non-ideal behavior of gas molecules.  One way to increase the non-ideal behavior of gas molecules under investigation would be to:

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11ecba2d_121e_b621_a3bf_2d813d6d73c3_MD0008_00 The first assumption made when modeling gas systems is that the gas molecules are ideal, with negligible molecular volume and no intermolecular forces. However, many real gas molecules do exert intermolecular forces on one another, and although molecular volume is very small, it is not zero. As a result, real gases exhibit deviations from ideal behavior. Attractive intermolecular interactions draw gas molecules toward the center of the container, decreasing the frequency of collisions with the container wall. Consequently, the ideal gas pressure (P_i) is always greater than the real pressure (P_r). This discrepancy is corrected by a term relating an attraction constant (a) to the square of the gas molecule density (n/V), which is the moles of gas (n) per unit of volume (V): 11ecba2d_121e_b622_a3bf_77a413233466_MD0008_00 Because every gas molecule occupies a non-negligible volume that diminishes the space through which the gas can move, ideal gas volume (V_i) is always less than real gas volume (V_r). This discrepancy is corrected by a term relating moles of gas (n) to a volume constant (b): 11ecba2d_121e_b623_a3bf_6b6d532a4e04_MD0008_00 The van der Waals equation is a restatement of the ideal gas equation with the correction terms added: 11ecba2d_121e_b624_a3bf_db9eb0b375b8_MD0008_00 The second assumption made when modeling gas systems is that gas molecules move freely throughout the system. However, high-pressure systems force gas molecules into close proximity, increasing the frequency of intermolecular interactions. Furthermore, low-temperature systems reduce the kinetic energy of gas molecules, decreasing the probability of molecules "escaping" intermolecular interactions. Therefore, deviations from ideal gas behavior are most often observed when gas molecules with non-negligible volume and significant intermolecular interactions are placed under conditions of high pressure and low temperature (Choice C). Conversely, non-ideal behavior of a real gas decreases when: Molecular volume is small, approximating the ideal model (Choice A). Decreases in pressure diminish the frequency of intermolecular interactions (Choice B). Increases in temperature diminish the longevity of intermolecular interactions (Choice D). Educational objective: Deviations from ideal gas behavior are observed when gas molecules with non-negligible volume and significant intermolecular interactions occupy a gas system at high pressure and low temperature.

A Scientist Uses Extreme Temperature Environments to Study the Non-Ideal