- What happens to the mean free path of gas molecules if the pressure is increased?
A) It increases.
B) It decreases.
C) It remains the same.
D) It becomes zero.
Answer: B) It decreases.
Explanation: Increasing pressure compresses the gas molecules closer together, leading to more frequent collisions and a shorter mean free path.
- The kinetic theory predicts that as the temperature of a gas increases, the distribution of molecular speeds:
A) Becomes narrower.
B) Becomes wider.
C) Remains unchanged.
D) Disappears.
Answer: B) Becomes wider.
Explanation: As temperature increases, molecules gain more kinetic energy, resulting in a wider range of speeds in the molecular speed distribution.
- The internal energy of an ideal diatomic gas is primarily due to:
A) Translational motion only.
B) Rotational and translational motion.
C) Vibrational motion only.
D) Chemical energy.
Answer: B) Rotational and translational motion.
Explanation: An ideal diatomic gas possesses kinetic energy from both translational and rotational motions, contributing to its internal energy.
- What does the term “thermal energy” refer to in the context of kinetic theory?
A) The total potential energy of gas molecules.
B) The average kinetic energy of gas molecules.
C) The energy transferred during a collision.
D) The energy associated with intermolecular forces.
Answer: B) The average kinetic energy of gas molecules.
Explanation: Thermal energy is primarily associated with the average kinetic energy of the molecules in a substance.
- The relationship between pressure and volume for a gas at constant temperature is represented by:
A) Charles’s Law.
B) Boyle’s Law.
C) Avogadro’s Law.
D) Ideal Gas Law.
Answer: B) Boyle’s Law.
Explanation: Boyle’s Law describes the inverse relationship between pressure and volume of a gas at constant temperature.
- In an ideal gas, the internal energy depends on:
A) Volume and pressure.
B) The number of moles and temperature.
C) Temperature only.
D) Molar mass only.
Answer: C) Temperature only.
Explanation: For an ideal gas, the internal energy is solely a function of temperature and does not depend on volume or pressure.
- Which of the following gases will have the highest root mean square speed at the same temperature?
A) Oxygen (O2)
B) Hydrogen (H2)
C) Nitrogen (N2)
D) Argon (Ar)
Answer: B) Hydrogen (H2)
Explanation: The root mean square speed is inversely proportional to the square root of molar mass, so hydrogen, being the lightest, has the highest speed.
- When two gases are mixed, the phenomenon of their spontaneous intermingling is called:
A) Compression.
B) Effusion.
C) Diffusion.
D) Expansion.
Answer: C) Diffusion.
Explanation: Diffusion is the process by which molecules of one gas spread out and mix with another gas.
- The law that describes the volume of a gas as directly proportional to its temperature at constant pressure is known as:
A) Boyle’s Law.
B) Charles’s Law.
C) Avogadro’s Law.
D) Dalton’s Law.
Answer: B) Charles’s Law.
Explanation: Charles’s Law states that the volume of a gas increases with an increase in temperature when pressure is held constant.
- The process by which gas molecules escape from a container through a small opening is called:
A) Diffusion.
B) Effusion.
C) Expansion.
D) Compression.
Answer: B) Effusion.
Explanation: Effusion refers to the process of gas escaping through a small hole, while diffusion is the mixing of gases.
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