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Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressure

Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressure

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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### Understanding the Behavior of Real Gases **Question:** Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. **Options:** (a) High pressure, small volume (b) High temperature, low pressure (c) Low temperature, high pressure **Explanation:** **(a) High Pressure, Small Volume:** Under high pressure and small volume, gas molecules are forced very close to each other. This scenario increases the intermolecular forces, causing significant deviations from ideal gas behavior. Real gases do not behave ideally under these conditions because the assumptions of negligible molecular volume and no intermolecular forces (key assumptions of the ideal gas law) no longer hold true. **(b) High Temperature, Low Pressure:** Real gases behave most like ideal gases at high temperatures and low pressures. At high temperatures, the kinetic energy of molecules is high, which diminishes the relative impact of intermolecular forces. Additionally, low pressure means that the molecules are far apart, reducing the effects of intermolecular forces and the volume of the gas molecules themselves. These conditions make real gases approximate the assumptions of the ideal gas law more closely. **(c) Low Temperature, High Pressure:** Under low temperature and high pressure, real gases deviate significantly from ideal behavior. At low temperatures, the kinetic energy of gas molecules decreases, making the intermolecular attractions more significant. High pressure forces the molecules closer together, further enhancing the impact of these attractions. Under these conditions, the behavior of the gas deviates substantially from the ideal gas model. **Conclusion:** - **Most Ideal Behavior:** Real gases behave most like ideal gases under conditions of **high temperature** and **low pressure** (Option b). - **Significant Deviation:** Real gases deviate significantly from ideal gas behavior under conditions of **high pressure** and **small volume** (Option a) and **low temperature** and **high pressure** (Option c).
Transcribed Image Text:### Understanding the Behavior of Real Gases **Question:** Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. **Options:** (a) High pressure, small volume (b) High temperature, low pressure (c) Low temperature, high pressure **Explanation:** **(a) High Pressure, Small Volume:** Under high pressure and small volume, gas molecules are forced very close to each other. This scenario increases the intermolecular forces, causing significant deviations from ideal gas behavior. Real gases do not behave ideally under these conditions because the assumptions of negligible molecular volume and no intermolecular forces (key assumptions of the ideal gas law) no longer hold true. **(b) High Temperature, Low Pressure:** Real gases behave most like ideal gases at high temperatures and low pressures. At high temperatures, the kinetic energy of molecules is high, which diminishes the relative impact of intermolecular forces. Additionally, low pressure means that the molecules are far apart, reducing the effects of intermolecular forces and the volume of the gas molecules themselves. These conditions make real gases approximate the assumptions of the ideal gas law more closely. **(c) Low Temperature, High Pressure:** Under low temperature and high pressure, real gases deviate significantly from ideal behavior. At low temperatures, the kinetic energy of gas molecules decreases, making the intermolecular attractions more significant. High pressure forces the molecules closer together, further enhancing the impact of these attractions. Under these conditions, the behavior of the gas deviates substantially from the ideal gas model. **Conclusion:** - **Most Ideal Behavior:** Real gases behave most like ideal gases under conditions of **high temperature** and **low pressure** (Option b). - **Significant Deviation:** Real gases deviate significantly from ideal gas behavior under conditions of **high pressure** and **small volume** (Option a) and **low temperature** and **high pressure** (Option c).
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