- According to Dalton’s Law of Partial Pressures, the total pressure of a mixture of gases is:
A) The difference of the partial pressures.
B) The sum of the partial pressures of individual gases.
C) The average of the partial pressures.
D) Independent of temperature.
Answer: B) The sum of the partial pressures of individual gases.
Explanation: Dalton’s Law states that the total pressure is equal to the sum of the partial pressures exerted by each component gas.
- When comparing two gases, if gas A is heavier than gas B, which of the following statements is true regarding their rates of diffusion?
A) Gas A diffuses faster than gas B.
B) Gas A and gas B diffuse at the same rate.
C) Gas B diffuses faster than gas A.
D) Diffusion rates cannot be compared.
Answer: C) Gas B diffuses faster than gas A.
Explanation: According to Graham’s Law, the rate of diffusion is inversely related to the square root of the molar mass; thus, the lighter gas (B) diffuses faster.
- The total energy of an ideal gas depends primarily on which of the following?
A) Pressure and volume.
B) Temperature and number of moles.
C) Molar mass and volume.
D) Pressure and temperature.
Answer: B) Temperature and number of moles.
Explanation: The total energy of an ideal gas is directly related to its temperature and the number of moles present.
- The law stating that the volume of a gas is directly proportional to its absolute temperature is known as:
A) Boyle’s Law.
B) Avogadro’s Law.
C) Charles’s Law.
D) Dalton’s Law.
Answer: C) Charles’s Law.
Explanation: Charles’s Law states that at constant pressure, the volume of a gas increases with an increase in absolute temperature.
- In which scenario does a real gas behave most ideally?
A) High pressure and low temperature.
B) Low pressure and high temperature.
C) Moderate pressure and temperature.
D) Low temperature and high density.
Answer: B) Low pressure and high temperature.
Explanation: Real gases behave more ideally under conditions of low pressure and high temperature, where intermolecular forces are minimized.
- The term “thermal energy” in gases primarily refers to:
A) Potential energy of molecules.
B) Kinetic energy of molecules.
C) Energy lost during collisions.
D) Energy stored in chemical bonds.
Answer: B) Kinetic energy of molecules.
Explanation: Thermal energy in gases is primarily associated with the kinetic energy of the gas molecules due to their motion.
- If a gas undergoes an isobaric expansion, which of the following remains constant?
A) Volume.
B) Pressure.
C) Temperature.
D) Internal energy.
Answer: B) Pressure.
Explanation: In an isobaric process, the pressure of the gas remains constant even as the volume changes.
- What is the primary assumption of the Kinetic Molecular Theory regarding gas molecules?
A) They attract each other strongly.
B) They are rigid and fixed in place.
C) They are in constant, random motion.
D) They have large volumes compared to the container.
Answer: C) They are in constant, random motion.
Explanation: One of the key assumptions of the Kinetic Molecular Theory is that gas molecules are always in random motion.
- The law that describes the relationship between pressure and the number of moles of a gas at constant temperature and volume is known as:
A) Boyle’s Law.
B) Charles’s Law.
C) Avogadro’s Law.
D) Dalton’s 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.
- Which of the following processes involves the transfer of energy without the movement of the medium?
A) Conduction.
B) Convection.
C) Radiation.
D) Advection.
Answer: A) Conduction.
Explanation: Conduction is the transfer of thermal energy through collisions between molecules without the movement of the medium itself.
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