Understanding Ideal and Real Gases

Which of the following is NOT an assumption of the ideal gas law?

• Gas particles experience significant intermolecular forces.

• Gas particles obey Newton's Laws of Motion.

• Collisions between gas particles are elastic.

• Gas particles have negligible volume.

What is a characteristic of a real gas that differentiates it from an ideal gas?

• Real gases have particles with negligible volume.

• Real gases only experience elastic collisions.

• Real gases have significant intermolecular forces.

• Real gases always obey Newton's Laws of Motion.

Why do real gases not behave ideally in a laboratory setting?

• Real gases always behave ideally.

• Real gases do not interact with each other.

• Real gases have no volume.

• Real gases have particles that interact in ways other than elastic collisions.

Under which conditions do real gases behave more like ideal gases?

• High temperatures and high pressures.

• High temperatures and low pressures.

• Low temperatures and high pressures.

• Low temperatures and low pressures.

What is the best approach to study a gas using the ideal gas law?

• Conduct experiments at high temperatures and high pressures.

• Conduct experiments at low temperatures and low pressures.

• Conduct experiments at low temperatures and high pressures.

• Conduct experiments at high temperatures and low pressures.