- If an ideal gas expands against a piston and does 500 J of work, how does this affect its internal energy?
A) Internal energy decreases
B) Internal energy increases
C) Internal energy remains the same
D) Internal energy fluctuates
Answer: A) Internal energy decreases
Explanation: In an isothermal process, the work done by the gas comes from its internal energy, resulting in a decrease in internal energy.
- Which of the following conditions would not typically be associated with ideal gas behavior?
A) Low pressure
B) High temperature
C) High density
D) Low intermolecular forces
Answer: C) High density
Explanation: High density typically indicates that intermolecular forces are significant, leading to deviations from ideal gas behavior.
- When two gases are mixed, how do their partial pressures relate to the total pressure?
A) They sum to the total pressure.
B) They multiply to give the total pressure.
C) They do not affect the total pressure.
D) They can be ignored.
Answer: A) They sum to the total pressure.
Explanation: According to Dalton’s Law of Partial Pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.
- What is the primary assumption of the Kinetic Molecular Theory regarding gas particles?
A) Gas particles occupy significant volume.
B) Gas particles are in constant, random motion.
C) Gas particles experience strong intermolecular forces.
D) Gas particles collide inelastically.
Answer: B) Gas particles are in constant, random motion.
Explanation: The Kinetic Molecular Theory assumes that gas particles are in continuous and random motion, which contributes to gas pressure.
- If a gas is compressed to a smaller volume while maintaining temperature, what must happen to the pressure?
A) Pressure decreases
B) Pressure remains constant
C) Pressure increases
D) Pressure fluctuates
Answer: C) Pressure increases
Explanation: According to Boyle’s Law, decreasing volume at constant temperature results in an increase in pressure.
- Which of the following statements about the Ideal Gas Law is true?
A) It applies to all gases under all conditions.
B) It is most accurate for real gases at low temperatures and high pressures.
C) It assumes no volume for gas particles.
D) It can only be used for monoatomic gases.
Answer: C) It assumes no volume for gas particles.
Explanation: The Ideal Gas Law assumes that gas particles have negligible volume and do not exert forces on each other.
- What happens to the average speed of gas molecules if the temperature is increased?
A) The average speed decreases
B) The average speed remains constant
C) The average speed increases
D) The average speed fluctuates
Answer: C) The average speed increases
Explanation: As temperature increases, the kinetic energy of gas molecules increases, leading to an increase in average speed.
- Which of the following conditions is not typically associated with gases behaving ideally?
A) High temperatures
B) Low pressures
C) Low intermolecular forces
D) High densities
Answer: D) High densities
Explanation: High densities suggest that gas molecules are closer together, increasing the effects of intermolecular forces, leading to non-ideal behavior.
- When the volume of a gas is increased, what happens to the number of moles if temperature and pressure are held constant?
A) Number of moles increases
B) Number of moles decreases
C) Number of moles remains constant
D) Number of moles fluctuates
Answer: C) Number of moles remains constant
Explanation: If both temperature and pressure are held constant, the number of moles of the gas remains unchanged regardless of volume changes.
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