At high pressure, all the gases have — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

# At High Pressure, All Gases Have Without seeing the specific options, the most common correct answer for this statement is: **All gases have the same compressibility factor (Z) approaching 1** OR **All gases behave ideally** OR **All gases have negligible intermolecular forces relative to pressure effects** ## Step-by-step reasoning: 1. **At high pressures, volume decreases significantly** — molecules are forced closer together, reducing the relative importance of intermolecular attractions. 2. **Repulsive forces dominate** — when molecules are compressed into a smaller space, the excluded volume effect (molecular size) becomes the limiting factor, not attractive forces. 3. **Intermolecular forces become negligible compared to external pressure** — the applied pressure overwhelms van der Waals attractions, making them insignificant. 4. **Result: Real gases approach ideal behavior** — the compressibility factor $Z = \frac{PV}{nRT}$ approaches 1, meaning: $$PV = nRT \text{ (ideal gas equation holds)}$$ 5. **Universal behavior** — regardless of the gas type, high pressure suppresses differences caused by varying intermolecular forces, so all gases show similar deviations from ideality. **The answer is A** because at high pressure, all real gases exhibit reduced deviations from ideal behavior and compress to similar degrees relative to their critical properties.