Kinetic Molecular Theory - AP Chemistry

1. What is the relationship between temperature and kinetic energy in gases?

   Kinetic energy is directly proportional to temperature in Kelvin. $KE \propto T$ where $T$ is in Kelvin scale.

2. According to Kinetic Molecular Theory, how do particles interact?

   Particles have no intermolecular forces. No attractions or repulsions between gas molecules.

3. What is the basic postulate of the Kinetic Molecular Theory regarding particle motion?

   Particles are in constant, random motion. This is the first fundamental postulate of kinetic theory.

4. Which option describes the kinetic molecular explanation for diffusion?

   Random motion allows particles to spread out over time. Random paths lead to net movement from high to low concentration.

5. What does Kinetic Molecular Theory assume about the direction of particle movement?

   Particles move in straight lines until collision. Linear motion between elastic collisions.

6. Which molecular property affects the speed of gas particles?

   Molar mass affects particle speed; heavier particles move slower. Lighter molecules move faster at same temperature.

7. Identify the property that remains constant for ideal gases according to Kinetic Molecular Theory.

   Average kinetic energy at constant temperature. At constant $T$, all gas particles have the same average $KE$.

8. What is the relationship between gas particle speed and temperature?

   Speed increases with temperature. Higher temperature means greater kinetic energy and velocity.

9. What happens to particle collisions with container walls as temperature increases?

   Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

10. How does the Kinetic Molecular Theory explain gas pressure?

    Pressure is due to collisions of particles with container walls. Moving particles strike walls, creating force per unit area.

11. What happens to the average kinetic energy of gas particles when the temperature is doubled?

    Average kinetic energy doubles. Kinetic energy directly proportional to temperature.

12. What modification in Kinetic Molecular Theory accounts for gas behavior at high pressures?

    Van der Waals equation accounts for particle volume. Corrects for finite molecular size at high pressure.

13. What is the relationship between gas pressure and temperature in a rigid container?

    Pressure is directly proportional to temperature. Gay-Lussac's law at constant volume.

14. What happens to gas particles when temperature increases, according to Kinetic Molecular Theory?

    Particles move faster as temperature increases. Higher $T$ means greater average kinetic energy and speed.

15. Describe the motion of gas particles according to Kinetic Molecular Theory.

    Rapid, random motion. Chaotic, high-speed movement in all directions.

16. How is the pressure of a gas affected when the temperature is halved at constant volume?

    Pressure is halved. Direct proportionality: $P \propto T$ at constant volume.

17. Explain how Kinetic Molecular Theory accounts for the compressibility of gases.

    Particles are far apart, allowing compression. Large spaces between molecules allow volume reduction.

18. What happens to particle collisions with container walls as temperature increases?

    Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

19. Which factor is directly proportional to the rate of effusion in gases?

    Inverse of the square root of molar mass. Graham's law: rate $\propto \frac{1}{\sqrt{M}}$.

20. What does Kinetic Molecular Theory assume about the direction of particle movement?

    Particles move in straight lines until collision. Linear motion between elastic collisions.

21. What happens to gas particle velocity distribution as temperature increases?

    Distribution broadens; average speed increases. Maxwell-Boltzmann distribution shifts to higher speeds.

22. Which gas law is derived from the Kinetic Molecular Theory?

    Ideal Gas Law: $PV = nRT$. Derived from kinetic theory assumptions about gas behavior.

23. According to Kinetic Molecular Theory, what assumption is made about gas particle attraction?

    No attractive forces between particles. Ideal gas assumption for simplified behavior.

24. What does Kinetic Molecular Theory assume about the direction of particle movement?

    Particles move in straight lines until collision. Linear motion between elastic collisions.

25. What happens to particle collisions with container walls as temperature increases?

    Collisions become more frequent and forceful. Higher kinetic energy leads to harder impacts.

26. What is the effect of decreasing temperature on the mean free path of gas particles?

    Mean free path decreases. Lower speed means less distance between collisions.

27. What assumption about particle volume is made in the Kinetic Molecular Theory?

    Particle volume is negligible compared to container volume. Point particles assumption for ideal gas behavior.

28. What is the effect of increased temperature on gas pressure, assuming volume is constant?

    Gas pressure increases as temperature increases. More collisions with walls due to faster particle motion.

29. According to Kinetic Molecular Theory, what is the effect of reducing volume on gas pressure at constant temperature?

    Pressure increases as volume decreases. Less space means more frequent wall collisions.

30. What is the effect of intermolecular forces on real gases compared to the ideal gas assumption?

    Real gases deviate due to intermolecular forces. Attractions reduce pressure; finite size affects volume.

31. Identify the assumption about gas particle collisions in the Kinetic Molecular Theory.

    Collisions are perfectly elastic. No energy lost in collisions for ideal gases.

32. Which parameter remains constant in an isothermal process according to the Kinetic Molecular Theory?

    Temperature remains constant. Isothermal means constant temperature process.

33. Which fundamental principle is used to derive the Ideal Gas Law from Kinetic Molecular Theory?

    Newton's laws of motion. Classical mechanics governs particle collisions and motion.

34. State the formula for calculating average kinetic energy of gas particles.

    $KE = \frac{3}{2} k T$. Where $k$ is Boltzmann constant and $T$ is temperature.

35. Identify the term for the average kinetic energy of gas particles.

    Thermal energy. Temperature is a measure of average kinetic energy.

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