Kinetic theory assumptions and pressure concept - One Line Questions

1. The pressure exerted by a gas is a macroscopic property that arises from the collective effect of: — Collisions of molecules with container walls.
2. If the number of moles of a gas is increased by a factor of 3, at constant volume and temperature, the pressure will: — Increase by a factor of 3.
3. The pressure exerted by an ideal gas is proportional to the total kinetic energy of the gas molecules per unit volume. If the volume is kept constant and the temperature is increased, the pressure will: — Increase.
4. Pressure in kinetic theory is fundamentally linked to the transfer of: — Momentum.
5. Which of the following is NOT an assumption of the kinetic theory of gases? — Collisions between molecules and with walls are inelastic.
6. Which of the following is a fundamental assumption of the kinetic theory of gases? — Gas molecules are perfectly elastic.
7. The pressure exerted by a gas is directly proportional to the number density (n/V) and the average kinetic energy of the molecules. If the number of molecules (N) is constant and the volume (V) is doubled, the pressure will: — Decrease.
8. The kinetic theory provides a microscopic explanation for the macroscopic gas laws, such as Boyle's Law, which states that at constant temperature, pressure is inversely proportional to volume. This is explained by: — Increased collision frequency with walls when volume decreases.
9. What type of collisions are assumed between gas molecules and the walls of the container in the kinetic theory? — Perfectly elastic collisions, conserving kinetic energy.
10. If the temperature of an ideal gas is increased, what happens to the average kinetic energy of its molecules? — It increases.
11. In the kinetic theory of gases, what is assumed about the volume of individual gas molecules? — It is negligible compared to the total volume occupied by the gas.
12. Which of the following statements about the mean free path in kinetic theory is correct? — It is the average distance traveled by a molecule between two successive collisions.
13. If the absolute temperature of an ideal gas is doubled, what happens to the rms speed of its molecules? — It increases by a factor of sqrt(2).
14. If the average kinetic energy of gas molecules is KE, the pressure exerted by the gas is proportional to: — KE
15. In the kinetic theory of gases, the molecules are assumed to be: — Point masses with no volume.
16. The kinetic theory of gases relates pressure to the momentum transfer during collisions. A higher frequency of collisions with the walls leads to: — Higher pressure.
17. Which assumption of kinetic theory is violated by real gases at very high pressures? — The volume of molecules is negligible.
18. Which assumption is particularly important for relating the macroscopic pressure to the microscopic motion of molecules? — Collisions are perfectly elastic.
19. Which assumption is crucial for deriving the ideal gas law from kinetic theory? — Collisions are perfectly elastic.
20. The kinetic theory explains that temperature is a measure of the average: — Kinetic energy of gas molecules.
21. The average distance between molecules in a gas is typically: — Much larger than the size of the molecules.
22. Which assumption is most critical for the temperature being directly proportional to the average kinetic energy? — Perfectly elastic collisions.
23. Which of the following factors does NOT affect the pressure exerted by an ideal gas, according to the kinetic theory of gases? — Mass of individual molecules.
24. The kinetic theory of gases assumes that the molecules possess: — Translational, rotational, and vibrational kinetic energies.
25. What is the primary characteristic of the motion of gas molecules according to the kinetic theory? — Random, chaotic motion.
26. What is the relationship between pressure (P) and the root-mean-square (rms) speed (v_rms) of gas molecules according to kinetic theory for an ideal gas? — P ∝ v_rms^2
27. The kinetic energy associated with the translational motion of gas molecules is given by (1/2)mv^2. The pressure is related to this kinetic energy by: — P is proportional to KE.
28. According to the kinetic theory, the internal energy of an ideal monatomic gas is solely due to: — Kinetic energy of translation.
29. If the volume of a container holding an ideal gas is halved, while temperature and number of moles are kept constant, how does the pressure change according to kinetic theory? — Pressure is doubled.
30. If the number of moles of an ideal gas in a container is doubled at constant volume and temperature, how does the pressure change? — Pressure is doubled.
31. What happens to the pressure of a gas if the mass of each molecule is doubled, while the number density and average speed remain constant? — Pressure remains the same.
32. If the average speed of gas molecules in a container is increased, what will happen to the pressure, assuming volume and number of molecules remain constant? — Pressure will increase.
33. Intermolecular forces between gas molecules are assumed to be negligible in the ideal gas model derived from kinetic theory, except during: — Collisions.
34. In the kinetic theory, the time taken for a collision between molecules is considered: — Negligible compared to the time between collisions.
35. In the kinetic theory, the time duration of a collision between gas molecules is assumed to be: — Zero, treated as instantaneous events.
36. The kinetic theory of gases models molecules as: — Point masses in constant, random motion.
37. The kinetic theory explains gas pressure as the result of: — The rate of change of momentum of molecules during collisions with walls.
38. According to the kinetic theory, the pressure exerted by a gas is directly proportional to: — The square of the average velocity of the molecules.
39. The pressure concept in kinetic theory is a consequence of: — The continuous bombardment of the container walls by molecules.
40. What does the term 'ideal gas' imply in the context of kinetic theory? — The gas molecules have no volume and no intermolecular forces.
41. According to the kinetic theory of gases, the pressure exerted by a gas is due to: — The collisions of gas molecules with the walls of the container.
42. The pressure exerted by an ideal gas is independent of: — The mass of individual molecules.
43. The concept of 'mean free path' is important in kinetic theory because it relates to: — The rate of diffusion and viscosity of the gas.
44. The average kinetic energy of gas molecules is directly proportional to: — The absolute temperature of the gas.
45. Which of the following statements is true about the intermolecular forces in the kinetic theory of gases? — They are negligible except during collisions.
46. What is assumed about the shape of gas molecules in the simplest kinetic theory model? — Their shape is irrelevant as they are treated as point masses.
47. What is the nature of the motion of gas molecules assumed in the kinetic theory? — Random and continuous.
48. The pressure of a gas is defined as force per unit: — Area.
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