Under which of the following conditions of temperature and pressure will H2 gas be expected to behav — States of Matter Chemistry Question

STEPS:

1. Identify the core assumptions of an ideal gas: An ideal gas is a theoretical model described by the Kinetic Molecular Theory (KMT). The model assumes that gas particles have negligible molecular volume compared to the total volume of their container, and that they experience no intermolecular attractions with one another.
2. Determine the conditions that minimize intermolecular attractions: Real gas molecules do exert weak attractive forces on one another. To minimize these attractions and behave more ideally, the gas must have high average kinetic energy so the molecules move too fast to be affected by attractive forces. This is achieved at high temperatures (500 K rather than 50 K).
3. Determine the conditions that minimize particle volume effects: Real gas molecules occupy a finite physical space. To make their individual molecular volumes negligible, the gas must be spread out over a very large container volume. This is achieved at low pressures (0.10 atm rather than 5.0 atm or 50 atm), where the distance between molecules is vast.
4. Select the optimal combination: Combining these two factors, a real gas behaves most like an ideal gas under high temperature and low pressure. Comparing the options, 500 K and 0.10 atm represents the highest temperature and lowest pressure, which corresponds to Option C.

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WHY_OTHERS_WRONG:

• A is incorrect: Although the pressure is low (0.10 atm), the temperature of 50 K is extremely low. At low temperatures, gas molecules move very slowly, allowing weak intermolecular attractions to significantly pull them together and cause a major deviation from ideal behavior.
• B is incorrect: This combination of low temperature (50 K) and high pressure (5.0 atm) represents the exact conditions under which real gases deviate *most* from ideal behavior. The molecules are packed closely together (making particle volume significant) and moving slowly (maximizing attractive forces).
• D is incorrect: Although the temperature is high (500 K), the pressure of 50 atm is far too high. Under extremely high pressures, the molecules are compressed into a tiny space where the physical volume of the gas particles themselves becomes a significant fraction of the container's volume.