- Which of the following is NOT a characteristic of an ideal gas?
A) No intermolecular forces.
B) Volume of gas particles is negligible.
C) Gas particles occupy a definite shape and volume.
D) Collisions between gas particles are elastic.
Answer: C) Gas particles occupy a definite shape and volume.
Explanation: Ideal gases are characterized by the lack of intermolecular forces and negligible volume of the particles, allowing them to expand and fill their container. They do not occupy a definite shape or volume.
- The relationship between pressure and temperature for a fixed amount of gas at constant volume is described by which law?
A) Boyle’s Law
B) Charles’s Law
C) Gay-Lussac’s Law
D) Avogadro’s Law
Answer: C) Gay-Lussac’s Law
Explanation: Gay-Lussac’s Law states that the pressure of a gas is directly proportional to its absolute temperature at constant volume. This can be expressed as
P∝T.
- Which of the following gases would you expect to behave most ideally?
A) Hydrogen
B) Carbon dioxide
C) Ammonia
D) Water vapor
Answer: A) Hydrogen
Explanation: Hydrogen is a light gas with weak intermolecular forces and occupies a small volume compared to other gases. It behaves most ideally under various conditions compared to heavier or more polar gases.
- If a gas is at a pressure of 2 atm and is expanded to a pressure of 1 atm while keeping the temperature constant, what happens to the volume of the gas?
A) It increases.
B) It decreases.
C) It remains constant.
D) It doubles.
Answer: A) It increases.
Explanation: According to Boyle’s Law, if the pressure decreases (from 2 atm to 1 atm) while keeping the temperature constant, the volume must increase.
- Which statement is true about gas behavior at extremely high pressures?
A) Gas behaves ideally.
B) Gas particles have no volume.
C) Intermolecular forces become significant.
D) The temperature decreases.
Answer: C) Intermolecular forces become significant.
Explanation: At high pressures, the volume of gas particles becomes significant compared to the total volume of the gas, and intermolecular forces start to affect the gas’s behavior, causing deviations from ideal gas behavior.
- What is the main assumption of the kinetic molecular theory regarding gas particles?
A) They are stationary.
B) They have strong intermolecular forces.
C) They are in constant random motion.
D) They occupy a fixed volume.
Answer: C) They are in constant random motion.
Explanation: The kinetic molecular theory states that gas particles are in continuous, random motion and that their collisions are elastic, which helps explain the properties of gases.
- According to Charles’s Law, if the volume of a gas is halved at constant pressure, what happens to the temperature?
A) It doubles.
B) It remains constant.
C) It is halved.
D) It decreases.
Answer: A) It doubles.
Explanation: Charles’s Law states that the volume of a gas is directly proportional to its temperature. Halving the volume at constant pressure would mean that the temperature must double to maintain the relationship.
- In a closed system, if the volume of a gas is tripled while keeping the temperature constant, what happens to the pressure?
A) It remains constant.
B) It triples.
C) It decreases to one-third.
D) It doubles.
Answer: C) It decreases to one-third.
Explanation: According to Boyle’s Law, if the volume increases, the pressure decreases inversely. Tripling the volume means the pressure will decrease to one-third of its original value.
- Which of the following factors does NOT affect the pressure of a gas in a container?
A) Temperature
B) Volume
C) Type of gas
D) Color of the container
Answer: D) Color of the container
Explanation: The color of the container does not influence the pressure of the gas inside it. Pressure is affected by temperature, volume, and the nature of the gas itself.
- Which gas law explains why helium-filled balloons shrink when exposed to cold temperatures?
A) Boyle’s Law
B) Charles’s Law
C) Gay-Lussac’s Law
D) Dalton’s Law
Answer: B) Charles’s Law
Explanation: Charles’s Law explains that as temperature decreases, the volume of gas also decreases when pressure is constant. This causes the helium in balloons to shrink in cold temperatures.
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