- The primary reason that gases can be compressed is due to:
A) Strong intermolecular forces.
B) The large distance between gas molecules.
C) High density of gases.
D) Low temperature.
Answer: B) The large distance between gas molecules.
Explanation: Gases can be compressed easily because the molecules are far apart, allowing for a significant reduction in volume when pressure is applied.
- The total kinetic energy of a gas is proportional to:
A) The number of molecules.
B) The volume of the gas.
C) The pressure of the gas.
D) Both A and C.
Answer: D) Both A and C.
Explanation: The total kinetic energy of a gas depends on the number of molecules and the temperature, which is related to the pressure in a closed system.
- Which of the following describes the conditions under which real gases behave most like ideal gases?
A) High pressure and low temperature.
B) High temperature and low pressure.
C) Low temperature and high density.
D) High density and low temperature.
Answer: B) High temperature and low pressure.
Explanation: Real gases behave more like ideal gases under conditions of high temperature and low pressure, where intermolecular forces are minimized.
- The gas law that relates volume and temperature at constant pressure is known as:
A) Boyle’s Law.
B) Charles’s Law.
C) Avogadro’s Law.
D) Graham’s Law.
Answer: B) Charles’s Law.
Explanation: Charles’s Law states that the volume of a gas is directly proportional to its absolute temperature when pressure is held constant.
- The mean free path is greater in:
A) High density gases.
B) Low density gases.
C) Gases at low temperatures.
D) Gases with larger molecular size.
Answer: B) Low density gases.
Explanation: The mean free path increases in low density gases because there are fewer molecules per unit volume, leading to fewer collisions.
- In a mixture of gases, each gas exerts pressure independently. This is a consequence of which principle?
A) Graham’s Law.
B) Dalton’s Law of Partial Pressures.
C) Boyle’s Law.
D) Charles’s Law.
Answer: B) Dalton’s Law of Partial Pressures.
Explanation: Dalton’s Law states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the partial pressures of each gas.
- The temperature of an ideal gas is directly related to:
A) The average potential energy of molecules.
B) The average kinetic energy of molecules.
C) The number of moles of gas.
D) The volume of the gas.
Answer: B) The average kinetic energy of molecules.
Explanation: The temperature of an ideal gas is a measure of the average kinetic energy of its molecules.
- If the volume of a gas is halved while the temperature is doubled, what happens to the pressure?
A) It remains the same.
B) It doubles.
C) It quadruples.
D) It halves.
Answer: C) It quadruples.
Explanation: According to the ideal gas law, if the volume is halved and the temperature is doubled, the pressure increases by a factor of four.
- The concept of “effusion” is best described as:
A) The process of gas mixing with another gas.
B) The process of gas escaping through a tiny opening.
C) The increase in volume of a gas.
D) The decrease in pressure of a gas.
Answer: B) The process of gas escaping through a tiny opening.
Explanation: Effusion specifically refers to the escape of gas molecules through a small hole into a vacuum.
- Which of the following is NOT an assumption of the kinetic theory of gases?
A) Gas molecules are in constant random motion.
B) Gas molecules occupy a significant volume.
C) Collisions between gas molecules are elastic.
D) There are no intermolecular forces between gas molecules.
Answer: B) Gas molecules occupy a significant volume.
Explanation: One of the key assumptions of the kinetic theory is that the volume of gas molecules is negligible compared to the volume of the gas itself.
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