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The derivation of the ideal gas equation employs two assumptions that are invalid for real gas molecules. First, the equation assumes that the molecules of the gas have no volume, which is not true for real molecules. Since the molecules will For carbon dioxide gas (CO2), the constants in the van der Waals equation are a = 0.364 J · m³ /moľ² and b= 4.27 × 10-5 m³ /mol. have some physical volume, the volume that the gas molecules occupy will be increased by the volume that the molecules occupy at rest. In addition, the equation ignores any interactions among the molecules. However, such interactions were first observed in the 19th century by J. D. van der Waals. He realized that, because of the intermolecular forces in the gas, there is a small but measurable attraction among the molecules, which will reduce the pressure of the gas on the walls of the container. To correct for these two deviations Part A If 1.00 mol of CO2 gas at 350 K is confined to a volume of 400 cm³, find the pressure pideal of the gas using the ideal gas equation. Express your answer numerically in pascals. • View Available Hint(s) from an ideal gas, the van der Waals equation gives (p+ an) (V – nb) = nRT, y? Pideal = Pa where a and b are empirical constants, which are different for different gasses. Submit Part B Find the pressure pydw of the gas using the van der Waals equation. Express your answer numerically in pascals.

The derivation of the ideal gas equation employs two assumptions that are invalid for real gas molecules. First, the equation assumes that the molecules of the gas have no volume, which is not true for real molecules. Since the molecules will For carbon dioxide gas (CO2), the constants in the van der Waals equation are a = 0.364 J · m³ /moľ² and b= 4.27 × 10-5 m³ /mol. have some physical volume, the volume that the gas molecules occupy will be increased by the volume that the molecules occupy at rest. In addition, the equation ignores any interactions among the molecules. However, such interactions were first observed in the 19th century by J. D. van der Waals. He realized that, because of the intermolecular forces in the gas, there is a small but measurable attraction among the molecules, which will reduce the pressure of the gas on the walls of the container. To correct for these two deviations Part A If 1.00 mol of CO2 gas at 350 K is confined to a volume of 400 cm³, find the pressure pideal of the gas using the ideal gas equation. Express your answer numerically in pascals. • View Available Hint(s) from an ideal gas, the van der Waals equation gives (p+ an) (V – nb) = nRT, y? Pideal = Pa where a and b are empirical constants, which are different for different gasses. Submit Part B Find the pressure pydw of the gas using the van der Waals equation. Express your answer numerically in pascals.

College Physics
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
Section: Chapter Questions
Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...
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Constants I Periodic Table The derivation of the ideal gas equation employs two assumptions that are invalid for real gas molecules. First, the equation assumes that the molecules of the gas have no volume, which is not true for real molecules. Since the molecules will For carbon dioxide gas (CO2), the constants in the van der Waals equation are a = = 0.364 J . m³ /mol and b = 4.27 x 10-5 m³ /mol. 3 have some physical volume, the volume that the gas molecules occupy will be increased by the volume that the molecules occupy at rest. In addition, the equation ignores any interactions among the molecules. However, such interactions were first observed in the 19th century by J. D. van der Waals. He realized that, because of the intermolecular forces in the gas, there is a small but measurable attraction among the molecules, which will reduce the pressure of the gas on the walls of the container. To correct for these two deviations Part A If 1.00 mol of CO2 gas at 350 K is confined to a volume of 400 cm³, find the pressure pideal of the gas using the ideal gas equation. Express your answer numerically in pascals. • View Available Hint(s) from an ideal gas, gives the van der Waals equation ΑΣφ an2 (p+ ) (V – nb) = nRT, V? Pideal = Ра where a and b are empirical constants, which are different for different gasses. Submit Part B Find the pressure pydw of the gas using the van der Waals equation. Express your answer numerically in pascals. View Available Hint(s)
Transcribed Image Text:Constants I Periodic Table The derivation of the ideal gas equation employs two assumptions that are invalid for real gas molecules. First, the equation assumes that the molecules of the gas have no volume, which is not true for real molecules. Since the molecules will For carbon dioxide gas (CO2), the constants in the van der Waals equation are a = = 0.364 J . m³ /mol and b = 4.27 x 10-5 m³ /mol. 3 have some physical volume, the volume that the gas molecules occupy will be increased by the volume that the molecules occupy at rest. In addition, the equation ignores any interactions among the molecules. However, such interactions were first observed in the 19th century by J. D. van der Waals. He realized that, because of the intermolecular forces in the gas, there is a small but measurable attraction among the molecules, which will reduce the pressure of the gas on the walls of the container. To correct for these two deviations Part A If 1.00 mol of CO2 gas at 350 K is confined to a volume of 400 cm³, find the pressure pideal of the gas using the ideal gas equation. Express your answer numerically in pascals. • View Available Hint(s) from an ideal gas, gives the van der Waals equation ΑΣφ an2 (p+ ) (V – nb) = nRT, V? Pideal = Ра where a and b are empirical constants, which are different for different gasses. Submit Part B Find the pressure pydw of the gas using the van der Waals equation. Express your answer numerically in pascals. View Available Hint(s)
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