Kinetic Theory of Temperature and Pressure - AP Physics 2

1. What is the molar volume of an ideal gas at STP?

   $22.4 \text{ L/mol}$. Standard molar volume for ideal gases.

2. Which gas law states that $PV/T$ is a constant for a given amount of gas?

   Combined Gas Law. Combines Boyle's, Charles's, and Gay-Lussac's laws.

3. What does Charles's Law state about temperature and volume?

   Volume is directly proportional to temperature. At constant pressure, $\frac{V}{T} = k$.

4. How does kinetic theory describe the energy distribution among particles?

   Energy is distributed according to a Maxwell-Boltzmann distribution. Statistical description of particle energies.

5. State the equation for Dalton's Law.

   $P_{total} = P_1 + P_2 + \text{...}$. Additive pressures in gas mixtures.

6. Calculate the pressure when a gas expands to double its volume at constant temperature.

   Pressure is halved. Application of Boyle's Law calculation.

7. What is the assumption about particle collisions in kinetic theory?

   Collisions are elastic. No energy lost in collisions.

8. Which variable remains constant in Boyle's Law?

   Temperature. Pressure and volume vary inversely.

9. What happens to particle speed as temperature increases?

   Particle speed increases. Higher temperature means more kinetic energy.

10. What is the definition of thermal equilibrium in kinetic theory?

    No net energy transfer between objects. Same temperature means equal average energies.

11. Define the term 'pressure' in the context of gases.

    Force exerted by gas particles per unit area. Molecular collisions create force.

12. What assumption about particle size is made in the kinetic theory of gases?

    Particles are point-like with negligible volume. Ideal gas approximation assumption.

13. What is the significance of the gas constant $R$?

    It relates energy units in the ideal gas law. Proportionality constant in gas equations.

14. What is the formula for kinetic energy of a gas particle?

    $KE = \frac{1}{2}mv^2$. Energy from mass and velocity squared.

15. What is the effect of temperature on the speed of sound in a gas?

    Speed of sound increases with temperature. Sound speed depends on molecular motion.

16. Identify the unit of temperature used in gas law calculations.

    Kelvin (K). Absolute temperature scale required.

17. State the relationship between pressure and volume in Boyle's Law.

    Pressure is inversely proportional to volume. At constant temperature, $PV = k$.

18. What happens to pressure if volume is halved at constant temperature?

    Pressure doubles. Inverse relationship from Boyle's Law.

19. What does Dalton's Law of Partial Pressures state?

    Total pressure is the sum of partial pressures. Each gas contributes independently.

20. If the pressure of a gas is tripled, what happens to its volume at constant temperature?

    Volume is reduced to one-third. Inverse pressure-volume relationship applied.

21. What is the value of the universal gas constant $R$?

    $8.314 \frac{J}{mol \times K}$. Standard value for gas calculations.

22. What causes gas pressure on a container's walls?

    Collisions of gas particles with the walls. Momentum transfer from particle impacts.

23. What is the equation for the ideal gas law?

    $PV = nRT$. Combines pressure, volume, moles, and temperature.

24. What is the equation for calculating density from pressure and temperature?

    $\rho = \frac{P \times M}{R \times T}$. Derived from ideal gas law rearrangement.

25. State the relationship between temperature and pressure in Gay-Lussac's Law.

    Pressure is directly proportional to temperature. At constant volume, $\frac{P}{T} = k$.

26. What is the relationship between temperature and kinetic energy?

    Kinetic energy is directly proportional to temperature. Temperature measures average kinetic energy.

27. What is the formula for calculating pressure?

    $P = \frac{F}{A}$. Force divided by contact area.

28. Identify the constant in Charles's Law.

    Pressure. Volume and temperature vary at fixed pressure.

29. What is the SI unit for pressure?

    Pascal (Pa). Newton per square meter.

30. What is the effect of lowering temperature on the kinetic energy of gas particles?

    Kinetic energy decreases. Temperature directly affects molecular energy.

31. What is Avogadro's Law in terms of volume and moles?

    Volume is directly proportional to moles. Equal volumes contain equal moles at STP.

32. What is the formula for converting Celsius to Kelvin?

    $K = C + 273.15$. Converts to absolute temperature scale.

33. Which law relates volume and amount of gas at constant temperature?

    Avogadro's Law. Volume proportional to gas quantity.

34. What does the kinetic theory of gases state about particle motion?

    Particles are in constant random motion. Foundation of kinetic molecular theory.

35. What is the formula for the number of moles $n$ in terms of mass $m$?

    $n = \frac{m}{M}$. Mass divided by molar mass gives moles.

36. What is the definition of absolute zero?

    The temperature at which particle motion stops. Zero kinetic energy at -273.15°C.

37. Define the term 'molar volume' at STP.

    The volume occupied by one mole of gas at STP. Standard volume at 0°C and 1 atm.

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