Any gas shows maximum deviation from ideal gas at — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

I'd be happy to help, but I notice the answer options (A, B, C, D) weren't included in your question. However, I can explain **when any gas shows maximum deviation from ideal behavior**: ## Key Concept: A gas deviates most from ideal behavior when **intermolecular forces are strongest and volume occupied by molecules is significant relative to container volume**. ## Conditions for Maximum Deviation: $$\text{Maximum deviation occurs at: } \boxed{\text{Low temperature and high pressure}}$$ **Why:** 1. **Low Temperature**: Kinetic energy decreases ($KE = \frac{3}{2}k_BT$), so intermolecular attractive forces dominate → greater deviation 2. **High Pressure**: Molecules are compressed closer together, making: - Excluded volume effect significant (real volume ≠ ideal volume) - Intermolecular attractions more pronounced 3. **Real vs Ideal**: The van der Waals equation shows: $$\left(P + \frac{a}{V_m^2}\right)(V_m - b) = RT$$ where $a$ accounts for attraction and $b$ for molecular volume. Both effects maximize at **low T and high P**. --- **If option C states "low temperature and high pressure"** or **"near critical point"**, that would be correct. Please share the options for a complete answer!