Under which of the following sets of conditions will a real gas most closely approach ideal behavior?

• A. High temperature and low pressure
• B. Low temperature and low pressure
• C. Low temperature and high pressure
• D. High temperature and high pressure

Answer: (A)

Verified step by step guidance

1. Recall that real gases deviate from ideal gas behavior due to intermolecular forces and the finite volume of gas particles.
2. Understand that at high temperatures, gas particles have more kinetic energy, which reduces the effect of intermolecular attractions and repulsions.
3. Recognize that at low pressures, gas particles are far apart, so the volume occupied by the particles themselves is negligible compared to the container volume, and intermolecular forces have less influence.
4. Combine these insights to conclude that a gas behaves most ideally under conditions of high temperature and low pressure, where both intermolecular forces and particle volume effects are minimized.
5. Therefore, among the given options, the set of conditions 'High temperature and low pressure' will make a real gas behave most like an ideal gas.