Under which of the following conditions do real gases behave most like ideal gases according to the kinetic molecular theory?

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

Answer: (B)

Verified step by step guidance

1. Recall that the kinetic molecular theory assumes gas particles have negligible volume and no intermolecular forces, which is best approximated under certain conditions.
2. Understand that at high temperatures, gas particles have more kinetic energy, which helps overcome intermolecular attractions, making the gas behave more ideally.
3. Recognize that at low pressures, gas particles are far apart, so their actual volume and interactions become less significant, aligning with ideal gas assumptions.
4. Combine these insights to conclude that gases behave most like ideal gases at high temperature and low pressure because particle volume and intermolecular forces are minimized.
5. Therefore, among the given options, the condition 'High temperature and low pressure' best fits the criteria for ideal gas behavior according to the kinetic molecular theory.