Question

Maximum deviation from ideal gas is expected from:

• A. $NH_3(g)$
• B. $H_3(g)$
• C. $N_2(g)$
• D. $CH_2(g)$

Hint:

The derivation of an ideal gas is dependent upon the Van der Waals constant.

Answer 1

The Correct Option is A

The question is about identifying the gas that shows the maximum deviation from ideal gas behavior among the given options. The deviation of gases from ideal behavior is explained by the intermolecular forces and volume of molecules, which are not considered in the ideal gas law. Real gases deviate from ideal gases at high pressures and low temperatures when the conditions approach condensation.

Let's analyze the options:

• $NH_3(g)$: Ammonia is a polar molecule with a significant dipole moment. The strong intermolecular hydrogen bonding in ammonia contributes to significant deviation from ideal gas behavior.
• $H_2(g)$: Hydrogen is a non-polar diatomic molecule with relatively weak Van der Waals forces, leading to minimal deviation from ideal behavior.
• $N_2(g)$: Nitrogen is also a non-polar diatomic molecule with little intermolecular attraction, thus showing minimal deviation.
• $CH_4(g)$: Methane, being a non-polar molecule, exhibits weak intermolecular forces, deviating minimally from ideal behavior.

The key here is recognizing that polar molecules like ammonia have stronger intermolecular forces (especially hydrogen bonds), which lead to larger deviations from ideal gas behavior than non-polar gases.

Conclusion: The maximum deviation from ideal gas behavior is expected from $NH_3(g)$ due to its polar nature and ability to form hydrogen bonds.