- Which of the following is true about the relationship between kinetic energy and temperature for an ideal gas?
A) Kinetic energy is independent of temperature.
B) Kinetic energy is inversely proportional to temperature.
C) Kinetic energy is directly proportional to temperature.
D) Kinetic energy depends on pressure only.
Answer: C) Kinetic energy is directly proportional to temperature.
Explanation: The average kinetic energy of gas molecules increases with an increase in temperature.
- In the context of kinetic theory, which of the following is true about gas molecules?
A) They have significant volume.
B) They are stationary.
C) They occupy the entire volume of the container.
D) They have strong intermolecular forces.
Answer: C) They occupy the entire volume of the container.
Explanation: Gas molecules are in constant motion and fill the entire volume of their container, unlike solids and liquids.
- The collision between gas molecules is described as:
A) Inelastic.
B) Elastic.
C) Perfectly inelastic.
D) Frictional.
Answer: B) Elastic.
Explanation: Collisions between gas molecules are considered perfectly elastic, meaning that total kinetic energy is conserved during the collisions.
- According to Graham’s law of effusion, the rate of effusion of a gas is inversely proportional to:
A) The square of its molar mass.
B) Its temperature.
C) Its pressure.
D) The square root of its molar mass.
Answer: D) The square root of its molar mass.
Explanation: Graham’s law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.
- What happens to the pressure of a gas when its temperature is doubled at constant volume?
A) Pressure halves.
B) Pressure remains constant.
C) Pressure doubles.
D) Pressure quadruples.
Answer: C) Pressure doubles.
Explanation: According to Gay-Lussac’s Law, if the temperature doubles while the volume remains constant, the pressure also doubles.
- The mean free path of gas molecules is affected by:
A) Temperature and pressure.
B) Volume only.
C) Density and temperature.
D) Only the type of gas.
Answer: A) Temperature and pressure.
Explanation: The mean free path increases with decreasing density (higher volume) and decreases with increasing temperature and pressure.
- Which of the following statements about real gases is true?
A) They always behave as ideal gases.
B) They exhibit attraction between molecules at low temperatures.
C) They occupy no volume.
D) Their behavior is independent of pressure.
Answer: B) They exhibit attraction between molecules at low temperatures.
Explanation: Real gases deviate from ideal behavior due to intermolecular forces, especially at low temperatures and high pressures.
- What is the effect of increasing the number of gas molecules in a container at constant volume and temperature?
A) Pressure increases.
B) Pressure decreases.
C) Volume decreases.
D) Temperature increases.
Answer: A) Pressure increases.
Explanation: Increasing the number of gas molecules while keeping volume and temperature constant increases the pressure due to more collisions with the walls of the container.
- The average speed of gas molecules increases with:
A) Decreasing temperature.
B) Increasing molar mass.
C) Increasing temperature.
D) Decreasing pressure.
Answer: C) Increasing temperature.
Explanation: The average speed of gas molecules is directly related to the temperature; higher temperatures mean more kinetic energy and higher speeds.
- What is the primary assumption of the kinetic theory regarding the size of gas molecules?
A) They are large compared to the container.
B) They have negligible volume compared to the total volume of the gas.
C) They are rigid.
D) They are significantly heavy.
Answer: B) They have negligible volume compared to the total volume of the gas.
Explanation: The kinetic theory assumes that the individual volume of gas molecules is negligible in comparison to the volume occupied by the gas as a whole.
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