Define an ideal gas.
A hypothetical gas that perfectly obeys the assumptions of the Kinetic Molecular Theory (KMT).
Define diffusion.
The mixing of gases due to the random motion of gas particles.
Define effusion.
The passage of a gas through a tiny hole into a vacuum.
What is the Kinetic Molecular Theory (KMT)?
A theory explaining gas behavior based on assumptions about particle motion and interactions.
What are intermolecular forces (IMFs)?
Attractive or repulsive forces between molecules.
What is the effect of increasing temperature on diffusion rate?
Increases the rate of diffusion.
What is the effect of increasing molecular size on diffusion rate?
Decreases the rate of diffusion.
What causes real gases to deviate from ideal behavior at low temperatures?
Attractive forces between gas particles become more significant.
What causes real gases to deviate from ideal behavior at high pressures?
The volume of gas particles becomes significant compared to the container volume.
What happens to the average kinetic energy of gas particles when temperature increases?
The average kinetic energy increases.
Compare diffusion and effusion.
Diffusion: Mixing of gases | Effusion: Gas passage through a small hole.
What are the key differences between real and ideal gases?
Ideal gases: Follow KMT assumptions perfectly. Real gases: Deviate, especially at low T and high P.
How does the volume of real gases compare to ideal gases?
Real gas volume is usually higher than ideal gas volume due to the significant volume of gas particles.
How does the pressure of real gases compare to ideal gases?
Real gas pressure is usually lower than ideal gas pressure due to attractive intermolecular forces.
Compare the rates of effusion of gases with different molar masses.
Lighter gases effuse faster than heavier gases.
