Questions on Kinetic Molecular Theory
Multiple-Choice Questions – Kinetic Molecular Theory
1. What does the Kinetic Molecular Theory primarily describe?
A) Chemical bonding in molecules
B) Behavior of gases
C) Atomic structure
D) Movement of electrons
E) Behavior of solids only
2. According to the Kinetic Molecular Theory, gas particles:
A) Move slowly and stick together
B) Are fixed in position
C) Move in random straight-line motion
D) Always repel each other
E) Move in circular orbits
3. In an ideal gas, the volume of individual gas particles is:
A) Zero
B) Large
C) Equal to the container
D) Constant but measurable
E) Increasing with pressure
4. The pressure exerted by a gas is due to:
A) The weight of the gas
B) Collisions of gas particles with the container walls
C) Chemical reactions
D) Attraction between gas particles
E) The number of moles
5. Which of the following is not an assumption of the Kinetic Molecular Theory?
A) Gas particles are in constant motion
B) Gas particles experience elastic collisions
C) Gas particles have negligible volume
D) Gas particles exert attractive forces
E) The average kinetic energy is proportional to temperature
6. What happens to the kinetic energy of gas particles when temperature increases?
A) It decreases
B) It becomes zero
C) It remains the same
D) It increases
E) It fluctuates randomly
7. According to KMT, gas particles collide:
A) Inelastically
B) With loss of energy
C) Without transferring energy
D) With elastic collisions
E) Rarely
8. Which condition makes a real gas behave most like an ideal gas?
A) Low temperature, high pressure
B) High temperature, low pressure
C) High density
D) Large molar mass
E) High polarity
9. What is directly proportional to the average kinetic energy of gas particles?
A) Volume
B) Mass
C) Pressure
D) Temperature in Kelvin
E) Molarity
10. In KMT, which factor does not influence gas pressure?
A) Volume of container
B) Number of particles
C) Temperature
D) Molar mass
E) Frequency of collisions
11. Gases with higher temperatures:
A) Have lower kinetic energy
B) Have slower particles
C) Have faster-moving particles
D) Occupy less volume
E) Exert no pressure
12. Kinetic energy of a gas particle depends on:
A) Its density
B) Its volume
C) Its color
D) Its mass and velocity
E) Its molar mass only
13. Real gases deviate most from ideal behavior at:
A) High temperature and low pressure
B) Low temperature and high pressure
C) STP
D) High temperature and high pressure
E) Low altitude
14. Why are gas particle collisions called "elastic"?
A) Because particles bounce off each other and lose energy
B) Because particles change shape
C) Because no kinetic energy is lost
D) Because gas volume increases
E) Because they occur rarely
15. The root mean square speed of a gas increases with:
A) Molar mass
B) Temperature
C) Pressure
D) Altitude
E) Volume
16. If two gases are at the same temperature, they:
A) Have the same mass
B) Have the same speed
C) Have the same kinetic energy
D) Have the same molar mass
E) Behave ideally
17. Which of the following statements is true regarding gas particles in the KMT?
A) They have strong intermolecular forces
B) They lose energy after collisions
C) They are constantly accelerating
D) They travel in straight lines until they collide
E) They rotate in place
18. The temperature at which gas particles theoretically have no motion is:
A) 0°C
B) -100°C
C) 273 K
D) 100°C
E) 0 K
19. In the Kinetic Molecular Theory, what causes temperature to rise?
A) Increased molar mass
B) Decrease in pressure
C) Increase in average kinetic energy
D) Expansion of the container
E) Decrease in volume
20. The KMT assumes gases have no intermolecular forces because:
A) It simplifies calculations
B) Gases are made of light particles
C) They are too small to exert force
D) Gases behave ideally under all conditions
E) Their volume cancels out the forces
- Questions on Gas Pressure
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Answers and Explanations
1. B – KMT explains the behavior of gases, including pressure and temperature relationships.
2. C – Gas particles move in random straight-line motion unless they collide.
3. A – In the ideal gas model, the volume of gas particles is negligible (zero).
4. B – Pressure results from collisions of gas molecules with container walls.
5. D – KMT assumes no attractive forces between particles.
6. D – Higher temperature = higher kinetic energy.
7. D – Collisions are elastic, meaning no net loss of kinetic energy.
8. B – High T, low P reduces intermolecular forces → ideal gas behavior.
9. D – Kinetic energy ∝ temperature (Kelvin).
10. D – Molar mass doesn't directly affect pressure in ideal gas law.
11. C – Faster-moving particles → higher T.
12. D – Kinetic energy depends on both mass and speed (velocity).
13. B – Real gases deviate most at low temperature and high pressure.
14. C – Elastic = no kinetic energy is lost during collisions.
15. B – Higher temperature → higher root mean square speed.
16. C – Same temperature → same average kinetic energy.
17. D – Gas particles move in straight lines until they collide.
18. E – 0 K is absolute zero, the point of no motion.
19. C – Temperature is related to kinetic energy.
20. A – Assumes no forces to simplify calculations and predict behavior.
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