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

💡 Solution & Explanation

# High Pressure Effects on Gases **Step 1: Understand the Real Gas Behavior** At high pressures, gases deviate from ideal behavior because intermolecular forces become significant and molecular volume becomes appreciable compared to container volume. **Step 2: Analyze Compressibility Factor (Z)** The compressibility factor is defined as: $$Z = \frac{PV}{nRT}$$ - For ideal gases: $Z = 1$ - For real gases at high pressure: $Z \neq 1$ (typically $Z < 1$ initially, then $Z > 1$ at very high pressures) **Step 3: Key Conclusion** At high pressures, all gases exhibit **similar compressibility factors** because: - Molecular volume effects dominate uniformly across different gases - Intermolecular repulsive forces become comparable - The ratio $\frac{PV}{nRT}$ converges toward similar values for different gases **Answer:** All gases have **similar (or the same) compressibility factor** at high pressures. This is the principle of the **law of corresponding states**—gases behave similarly when compared at reduced conditions (reduced pressure, volume, and temperature), which becomes particularly evident at high absolute pressures.