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A gas will behave ideally at: O high pressure and high temperature O low pressure and high temperature O high pressure and low temperature O low pressure and low temperature

A gas will behave ideally at: O high pressure and high temperature O low pressure and high temperature O high pressure and low temperature O low pressure and low temperature

Chemistry
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Understanding Ideal Gas Behavior In this section, we explore the conditions under which a gas behaves most ideally. This knowledge is crucial for understanding gas laws and their applications in various scientific fields. #### Multiple Choice Question: Ideal Gas Conditions A gas will behave ideally at: - ⃝ high pressure and high temperature - ⃝ low pressure and high temperature - ⃝ high pressure and low temperature - ⃝ low pressure and low temperature **Explanation:** - **High pressure and high temperature:** Under high pressure, gas molecules are forced into close proximity, making intermolecular forces more significant, which deviates from ideal gas behavior. - **Low pressure and high temperature:** At low pressure, gas molecules are far apart, reducing intermolecular forces. High temperature provides sufficient kinetic energy to overcome any attractive forces, making this the most ideal condition for gas behavior. - **High pressure and low temperature:** High pressure and low temperature both lead to significant intermolecular forces, causing deviations from ideal gas laws. - **Low pressure and low temperature:** While low pressure minimizes intermolecular forces, low temperature reduces the kinetic energy of gas molecules, potentially allowing attractive forces to become significant. #### Conclusion For a gas to behave ideally, it must be subjected to **low pressure and high temperature**. This condition ensures minimal intermolecular forces and sufficient kinetic energy for the gas molecules, closely aligning with the assumptions of the ideal gas law. --- **Note:** If you encounter any graphs or diagrams in this section, we would typically provide detailed explanations of each component. However, this question does not include any visual aids, focusing instead on conceptual understanding.
Transcribed Image Text:### Understanding Ideal Gas Behavior In this section, we explore the conditions under which a gas behaves most ideally. This knowledge is crucial for understanding gas laws and their applications in various scientific fields. #### Multiple Choice Question: Ideal Gas Conditions A gas will behave ideally at: - ⃝ high pressure and high temperature - ⃝ low pressure and high temperature - ⃝ high pressure and low temperature - ⃝ low pressure and low temperature **Explanation:** - **High pressure and high temperature:** Under high pressure, gas molecules are forced into close proximity, making intermolecular forces more significant, which deviates from ideal gas behavior. - **Low pressure and high temperature:** At low pressure, gas molecules are far apart, reducing intermolecular forces. High temperature provides sufficient kinetic energy to overcome any attractive forces, making this the most ideal condition for gas behavior. - **High pressure and low temperature:** High pressure and low temperature both lead to significant intermolecular forces, causing deviations from ideal gas laws. - **Low pressure and low temperature:** While low pressure minimizes intermolecular forces, low temperature reduces the kinetic energy of gas molecules, potentially allowing attractive forces to become significant. #### Conclusion For a gas to behave ideally, it must be subjected to **low pressure and high temperature**. This condition ensures minimal intermolecular forces and sufficient kinetic energy for the gas molecules, closely aligning with the assumptions of the ideal gas law. --- **Note:** If you encounter any graphs or diagrams in this section, we would typically provide detailed explanations of each component. However, this question does not include any visual aids, focusing instead on conceptual understanding.
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