Which of the following properties applies to an ideal gas according to the ideal gas law?

• A. The gas particles have negligible volume.
• B. The gas volume decreases as temperature increases at constant pressure.
• C. The gas pressure is independent of temperature.
• D. The gas particles experience strong intermolecular forces.

Answer: (A)

Verified step by step guidance

1. Recall the assumptions of the ideal gas law, which models gases under ideal conditions. These assumptions include that gas particles have negligible volume and do not exert intermolecular forces on each other.
2. Understand that the ideal gas law is given by the equation \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is moles of gas, \(R\) is the gas constant, and \(T\) is temperature in Kelvin.
3. Analyze each statement in the problem: - 'The gas particles have negligible volume' aligns with the ideal gas assumption that particles are point-like with no volume. - 'The gas volume decreases as temperature increases at constant pressure' contradicts Charles's Law, which states volume increases with temperature at constant pressure. - 'The gas pressure is independent of temperature' contradicts Gay-Lussac's Law, which states pressure increases with temperature at constant volume. - 'The gas particles experience strong intermolecular forces' contradicts the ideal gas assumption of no intermolecular forces.
4. Conclude that the only property consistent with the ideal gas law assumptions is that gas particles have negligible volume.
5. Remember that deviations from ideal gas behavior occur when gas particles have significant volume or experience intermolecular forces, which are not accounted for in the ideal gas law.