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

💡 Solution & Explanation

# Maximum Deviation from Ideal Gas Behavior **Step 1: Understand when gases deviate from ideality** Real gases deviate from ideal behavior due to: - Intermolecular forces (van der Waals attractions) - Finite molecular volume **Step 2: Identify conditions favoring maximum deviation** Deviations are maximized when: - **Low temperature** → molecules move slowly, intermolecular forces dominate - **High pressure** → molecules are close together, molecular volume becomes significant $$\text{Deviation} \propto \frac{1}{T} \text{ and } \propto P$$ **Step 3: Apply van der Waals equation** The correction factors show why: $$\left(P + \frac{a}{V^2}\right)(V - b) = RT$$ - Term $\frac{a}{V^2}$ (attraction): largest at low $T$ and high $P$ - Term $b$ (volume): most significant at high $P$ **Step 4: Conclude** **Answer C: Low temperature and high pressure** Any gas shows **maximum deviation** at **low temperature** (molecules interact longer) and **high pressure** (molecules crowded together, excluded volume matters). --- *Note: Without seeing the options, option C typically represents "low temperature and high pressure" in standard chemistry courses.*