- If a gas has a molar mass of 32 g/mol and another gas has a molar mass of 16 g/mol, which gas will diffuse faster at the same temperature?
A) The gas with 32 g/mol.
B) The gas with 16 g/mol.
C) Both gases will diffuse at the same rate.
D) It cannot be determined.
Answer: B) The gas with 16 g/mol.
Explanation: According to Graham’s Law, the rate of diffusion is inversely proportional to the square root of the molar mass. Thus, the lighter gas (16 g/mol) will diffuse faster than the heavier gas (32 g/mol).
- When discussing gas behavior, what does the term “real gas” refer to?
A) A gas that behaves according to the ideal gas law.
B) A gas that behaves similarly to an ideal gas under all conditions.
C) A gas that deviates from ideal gas behavior due to intermolecular forces.
D) A gas that has a constant volume and pressure.
Answer: C) A gas that deviates from ideal gas behavior due to intermolecular forces.
Explanation: Real gases exhibit behaviors that deviate from ideal gas laws, particularly under high pressure and low temperature where intermolecular forces become significant.
- Which of the following statements describes the relationship between temperature and kinetic energy of gas particles?
A) They are inversely related.
B) They are directly related.
C) They are independent of each other.
D) They have no relationship.
Answer: B) They are directly related.
Explanation: The temperature of a gas is directly proportional to the average kinetic energy of its particles; as temperature increases, the kinetic energy also increases.
- What happens to the density of a gas if its temperature is increased while keeping the pressure constant?
A) It increases.
B) It decreases.
C) It remains constant.
D) It becomes zero.
Answer: B) It decreases.
Explanation: Increasing the temperature of a gas at constant pressure causes its volume to increase, which results in a decrease in density (density = mass/volume).
- Which gas law can be used to determine the relationship between the amount of gas and its volume?
A) Boyle’s Law
B) Charles’s Law
C) Avogadro’s Law
D) Ideal Gas Law
Answer: C) Avogadro’s Law
Explanation: Avogadro’s Law states that the volume of a gas is directly proportional to the number of moles of gas at constant temperature and pressure.
- If a gas in a balloon is compressed, what will happen to the temperature if the compression occurs rapidly and no heat is exchanged?
A) The temperature decreases.
B) The temperature increases.
C) The temperature remains constant.
D) The gas escapes.
Answer: B) The temperature increases.
Explanation: Rapid compression does work on the gas, which increases the kinetic energy of the gas particles and thus raises the temperature.
- When considering gas laws, what does the term “absolute zero” refer to?
A) The lowest temperature possible where gas particles are at rest.
B) A temperature where all gases behave ideally.
C) A point where gas volume is maximized.
D) A theoretical temperature where pressure is infinite.
Answer: A) The lowest temperature possible where gas particles are at rest.
Explanation: Absolute zero is defined as 0 Kelvin (-273.15°C), where gas particles theoretically have minimal kinetic energy and are at rest.
- In a closed container, if the volume is halved and the temperature is kept constant, what will happen to the pressure?
A) It will halve.
B) It will double.
C) It will triple.
D) It will remain the same.
Answer: B) It will double.
Explanation: According to Boyle’s Law, halving the volume while keeping temperature constant results in a doubling of pressure.
- The relationship between pressure and volume of a gas at constant temperature is represented by which law?
A) Charles’s Law
B) Gay-Lussac’s Law
C) Boyle’s Law
D) Avogadro’s Law
Answer: C) Boyle’s Law
Explanation: Boyle’s Law describes the inverse relationship between pressure and volume at constant temperature.
- Which of the following is a key assumption of the ideal gas model?
A) Gas particles are stationary.
B) Gas particles have a significant volume.
C) There are no intermolecular forces between gas particles.
D) Gas behavior does not change with temperature.
Answer: C) There are no intermolecular forces between gas particles.
Explanation: A key assumption of the ideal gas model is that gas particles do not exert attractive or repulsive forces on one another, allowing them to behave ideally.
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