- What is the relationship between the kinetic energy of gas molecules and temperature in Kelvin?
A) Directly proportional
B) Inversely proportional
C) No relationship
D) Exponential
Answer: A) Directly proportional
Explanation: The average kinetic energy of gas molecules is directly proportional to the absolute temperature in Kelvin.
- In the context of the Ideal Gas Law, what does the term “ideal gas” refer to?
A) A gas that can be easily liquefied
B) A gas that behaves according to the Ideal Gas Law under all conditions
C) A gas that has zero volume and no intermolecular forces
D) A gas that does not exist in nature
Answer: C) A gas that has zero volume and no intermolecular forces
Explanation: An ideal gas is a theoretical construct used to describe a gas whose molecules occupy no volume and have no intermolecular forces.
- Which gas law would you use to calculate the change in pressure of a gas if its temperature changes but its volume remains constant?
A) Boyle’s Law
B) Charles’s Law
C) Gay-Lussac’s Law
D) Dalton’s Law
Answer: C) Gay-Lussac’s Law
Explanation: Gay-Lussac’s Law relates the pressure of a gas to its temperature when volume is constant.
- What is the effect on gas pressure if the volume is increased while the temperature and the number of moles remain constant?
A) Pressure increases
B) Pressure decreases
C) Pressure remains constant
D) Pressure fluctuates
Answer: B) Pressure decreases
Explanation: According to Boyle’s Law, if the volume increases at constant temperature, the pressure must decrease.
- The behavior of real gases can be modeled more accurately using which equation?
A) Ideal Gas Equation
B) Van der Waals Equation
C) Charles’s Law
D) Boyle’s Law
Answer: B) Van der Waals Equation
Explanation: The Van der Waals Equation includes corrections for intermolecular forces and molecular volume, providing a more accurate description of real gas behavior.
- In which scenario would a real gas behave most like an ideal gas?
A) Low temperature, high pressure
B) High temperature, low pressure
C) Low temperature, low pressure
D) High temperature, high pressure
Answer: B) High temperature, low pressure
Explanation: High temperatures and low pressures minimize the effects of intermolecular forces, causing the gas to behave more ideally.
- If the molar mass of a gas is increased, what happens to its density at constant temperature and pressure?
A) Density increases
B) Density decreases
C) Density remains constant
D) Density fluctuates
Answer: A) Density increases
Explanation: Density is directly proportional to molar mass; thus, if molar mass increases, density also increases at constant temperature and pressure.
- If a gas expands against a constant external pressure, what type of work is done?
A) Positive work
B) Negative work
C) Zero work
D) Internal work
Answer: A) Positive work
Explanation: When a gas expands, it does work on the surroundings, which is considered positive work in thermodynamics.
- Which property of a gas is represented by the symbol V in the Ideal Gas Equation?
A) Volume
B) Velocity
C) Viscosity
D) Vapor pressure
Answer: A) Volume
- When using the Ideal Gas Law, what is the standard pressure value typically used?
A) 1 atm
B) 760 mmHg
C) 101.3 kPa
D) All of the above
Answer: D) All of the above
Explanation: 1 atm, 760 mmHg, and 101.3 kPa are all equivalent measures of standard pressure.
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