Compared to a real gas, how does an ideal gas behave at very high pressures_________________?
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Answer: A. more volume
Explanation
Intermolecular repulsive forces dominate real gases at very high pressures, expanding their volume. Real gas molecules occupy finite physical space, unlike idealized point-mass assumptions. Consequently, real gases deviate from ideal gas laws by exhibiting larger actual volumes. The ideal gas law assumes negligible molecular volume and zero intermolecular attractive forces. Van der Waals equations correct for molecular volume and intermolecular forces at high pressures. Compressibility factors quantify how much real gases deviate from ideal behavior under extreme conditions.
High-pressure gas storage vessel design requires real gas corrections to predict container sizing accurately. Chemical engineering processes operating at high pressures must account for volumetric deviations. Failing to use real gas equations at high pressures leads to significant operational safety errors. Option B incorrectly suggests real gases compress to smaller volumes than ideal predictions. Option C ignores well-documented compressibility deviations occurring at high pressure extremes. Option D is false because real gas behavior under high pressure follows predictable scientific principles.
- Subject
- Engineering
- Category
- Mechanical Engineering
- Topic
- —
- Difficulty
- medium
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