- Which factor does NOT influence the behavior of an ideal gas?
A) Temperature
B) Volume
C) The nature of the gas
D) Pressure
Answer: C) The nature of the gas
Explanation: In ideal gas behavior, the nature of the gas (i.e., its identity) does not influence the ideal gas law directly, as ideal gases are defined by their properties without considering the specific type of gas.
- When a gas is allowed to expand adiabatically, which of the following is true?
A) Heat is absorbed from the surroundings.
B) Heat is released to the surroundings.
C) No heat is exchanged with the surroundings.
D) The temperature of the gas increases.
Answer: C) No heat is exchanged with the surroundings.
Explanation: In an adiabatic process, there is no heat exchange with the surroundings, meaning the system is insulated.
- In a sealed container, if the temperature of a gas decreases, what happens to its pressure?
A) It increases.
B) It remains constant.
C) It decreases.
D) It becomes zero.
Answer: C) It decreases.
Explanation: According to Gay-Lussac’s Law, if the temperature of a gas decreases at constant volume, the pressure will also decrease.
- Which of the following conditions best allows for ideal gas behavior?
A) Low temperature and high pressure.
B) Low temperature and low pressure.
C) High temperature and low pressure.
D) High pressure and low temperature.
Answer: C) High temperature and low pressure.
Explanation: High temperatures and low pressures reduce the effects of intermolecular forces and the volume occupied by gas particles, allowing gases to behave more ideally.
- The combined gas law combines which of the following laws?
A) Boyle’s Law, Charles’s Law, and Avogadro’s Law
B) Boyle’s Law and Charles’s Law
C) Boyle’s Law, Gay-Lussac’s Law, and Charles’s Law
D) Ideal Gas Law and Dalton’s Law
Answer: C) Boyle’s Law, Gay-Lussac’s Law, and Charles’s Law
Explanation: The combined gas law relates pressure, volume, and temperature in a single equation by combining Boyle’s Law, Gay-Lussac’s Law, and Charles’s Law.
- In a closed system, if the volume of a gas decreases, what must happen to the temperature for the pressure to remain constant?
A) It must increase.
B) It must decrease.
C) It must remain constant.
D) It must double.
Answer: A) It must increase.
Explanation: According to the ideal gas law, if the volume decreases while pressure is to remain constant, the temperature must increase.
- When considering the kinetic molecular theory, which of the following statements is NOT true?
A) Gas particles are in constant random motion.
B) Gas particles occupy a negligible volume compared to the container’s volume.
C) Gas particles exert no forces on each other.
D) Gas particles have strong attractive forces between them.
Answer: D) Gas particles have strong attractive forces between them.
Explanation: According to the kinetic molecular theory, gas particles are assumed to have negligible intermolecular forces, allowing them to behave ideally.
- A gas has a volume of 10 L at a pressure of 2 atm. If the volume is reduced to 5 L at constant temperature, what will be the new pressure?
A) 1 atm
B) 2 atm
C) 4 atm
D) 8 atm
Answer: C) 4 atm
Explanation: According to Boyle’s Law, if the volume is halved (from 10 L to 5 L), the pressure will double (from 2 atm to 4 atm).
- What happens to the pressure of a gas if it is compressed to a smaller volume while keeping the temperature constant?
A) It decreases.
B) It remains the same.
C) It increases.
D) It becomes zero.
Answer: C) It increases.
Explanation: According to Boyle’s Law, if the volume of a gas decreases while the temperature remains constant, the pressure will increase.
- If a gas is compressed to half its volume, what happens to the temperature if the pressure is kept constant?
A) It decreases.
B) It increases.
C) It remains the same.
D) It becomes zero.
Answer: B) It increases.
Explanation: According to Charles’s Law, if the volume is halved at constant pressure, the temperature must increase to maintain the gas laws.
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