Kinetic Molecular Theory Trivia Quiz
these questions deal with kinetic molecular theory as well as ideal gases. check it out.
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you must score at least 70
- 1.
Which gas sample at STP has the same total number of molecules as 2.0 liters of CO2 (g) at STP?
- A.
5.0 L of CO2 (g)
- B.
2.0 L of Cl2 (g)
- C.
3.0 L of H2S (g)
- D.
6.0 L of He (g)
Correct Answer
B. 2.0 L of Cl2 (g)Explanation
The number of molecules in a gas sample can be determined using Avogadro's Law, which states that equal volumes of gases at the same temperature and pressure contain the same number of molecules. Since the question specifies that the gases are at STP (standard temperature and pressure), we can compare the volumes of the gases to determine which one has the same number of molecules as 2.0 liters of CO2. Therefore, the correct answer is 2.0 L of Cl2 (g).Rate this question:
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- 2.
A gas sample is at STP. Which changes in temperature and pressure will cause this sample to behave more like an ideal gas?
- A.
Decreased temperature and increased pressure
- B.
Decreased temperature and decreased pressure
- C.
Increased temperature and increased pressure
- D.
Increased temperature and decreased pressure
Correct Answer
D. Increased temperature and decreased pressureExplanation
When the temperature of a gas sample is increased, the kinetic energy of the gas particles also increases. This causes the gas particles to move faster and collide more frequently with each other and the walls of the container. As a result, the gas sample behaves more like an ideal gas, where the gas particles are assumed to have negligible volume and no intermolecular forces.
On the other hand, when the pressure of a gas sample is decreased, the gas particles have more space to move around and collide with each other. This reduces the likelihood of intermolecular interactions and deviations from ideal gas behavior. Therefore, the combination of increased temperature and decreased pressure will cause the gas sample to behave more like an ideal gas.Rate this question:
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- 3.
Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas?
- A.
100 K and 0.25 atm
- B.
100 K and 25 atm
- C.
400 K and 0.25 atm
- D.
400 K and 25 atm
Correct Answer
C. 400 K and 0.25 atmExplanation
At higher temperatures and lower pressures, gases tend to behave more like ideal gases. This is because at higher temperatures, the kinetic energy of the gas particles increases, causing them to move faster and collide more frequently, resulting in a more random and uniform distribution of particles. At lower pressures, the intermolecular forces between the gas particles become less significant compared to the kinetic energy, allowing the gas particles to move more freely and independently. Therefore, at 400 K and 0.25 atm, the sample of neon is most likely to behave like an ideal gas.Rate this question:
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- 4.
According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas?
- A.
The force of attraction between the gas particles is strong.
- B.
The motion of the gas particles is random and straight-line.
- C.
The collisions between the gas particles cannot result in a transfer of energy between the particles.
- D.
The separation between the gas particles is smaller than the size of the gas particles themselves.
Correct Answer
B. The motion of the gas particles is random and straight-line.Explanation
The statement that describes the particles in a sample of an ideal gas according to the kinetic molecular theory is that the motion of the gas particles is random and straight-line. This means that the particles move in all directions with no preferred direction and they travel in straight lines until they collide with other particles or the walls of the container. This behavior is explained by the concept of kinetic energy and the assumption that gas particles are in constant motion.Rate this question:
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- 5.
Under which conditions of temperature and pressure does oxygen gas behave most like an ideal gas?
- A.
Low temperature and low pressure
- B.
Low temperature and high pressure
- C.
High temperature and low pressure
- D.
High temperature and high pressure
Correct Answer
C. High temperature and low pressureExplanation
Oxygen gas behaves most like an ideal gas under high temperature and low pressure conditions. At high temperatures, the kinetic energy of the gas particles increases, causing them to move more rapidly and collide more frequently. This results in a more random and chaotic motion, which is a characteristic of an ideal gas. Additionally, at low pressures, the intermolecular forces between oxygen gas particles are weaker, allowing them to behave more like independent particles with negligible interactions.Rate this question:
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- 6.
Under which conditions of temperature and pressure would helium behave most like an ideal gas?
- A.
50K and 20kPa
- B.
50K and 600kPa
- C.
750K and 20kPa
- D.
750K and 600kPa
Correct Answer
C. 750K and 20kPaExplanation
At higher temperatures and lower pressures, gases tend to behave more like ideal gases. This is because at higher temperatures, the kinetic energy of the gas particles increases, causing them to move more rapidly and collide with each other less frequently. At lower pressures, the gas particles are more spread out, resulting in fewer intermolecular interactions. Therefore, the conditions of 750K and 20kPa would make helium behave most like an ideal gas.Rate this question:
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- 7.
A real gas behaves more like an ideal gas when the gas molecules are
- A.
Close and have strong attractive forces between them
- B.
Close and have weak attractive forces between them
- C.
Far apart and have strong attractive forces between them
- D.
Far apart and have weak attractive forces between them
Correct Answer
D. Far apart and have weak attractive forces between themExplanation
When gas molecules are far apart and have weak attractive forces between them, they are able to move more freely and independently. This is similar to the behavior of ideal gases, which are assumed to have no intermolecular forces and occupy no volume. In contrast, when gas molecules are close together and have strong attractive forces between them, they are more likely to deviate from ideal gas behavior and exhibit properties such as condensation and liquefaction. Therefore, the statement suggests that a real gas behaves more like an ideal gas when the gas molecules are far apart and have weak attractive forces between them.Rate this question:
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- 8.
The concept of an ideal gas is used to explain
- A.
The mass of a gas sample
- B.
The behavior of a gas sample
- C.
Why some gases are monatomic
- D.
Why some gases are diatomic
Correct Answer
B. The behavior of a gas sampleExplanation
The concept of an ideal gas is used to explain the behavior of a gas sample. The behavior of a gas sample refers to its properties, such as pressure, volume, and temperature, and how these properties are related to each other. The ideal gas law, which is based on the concept of an ideal gas, describes the relationship between these properties and allows us to predict and explain the behavior of gases under different conditions.Rate this question:
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- 9.
According to the kinetic molecular theory, the particles of an ideal gas
- A.
Have no potential energy
- B.
Have strong intermolecular forces
- C.
Are arranged in a regular, repeated geometric pattern
- D.
Are separated by great distances, compared to their size
Correct Answer
D. Are separated by great distances, compared to their sizeExplanation
According to the kinetic molecular theory, the particles of an ideal gas are separated by great distances, compared to their size. This means that the particles are not closely packed together, but rather spread out. This is because the particles in an ideal gas are in constant motion and move freely in all directions. The large distances between the particles allow them to move independently and collide with each other and the walls of the container. This is why gases are able to expand and fill the entire volume of their container.Rate this question:
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- 10.
The kinetic molecular theory assumes that the particles of an ideal gas
- A.
Are in random, constant, straight-line motion
- B.
Are arranged in a regular geometric pattern
- C.
Have strong attractive forces between them
- D.
Have collisions that result in the system losing energy
Correct Answer
A. Are in random, constant, straight-line motionExplanation
The kinetic molecular theory assumes that the particles of an ideal gas are in random, constant, straight-line motion. This means that the particles move in a random manner, with no specific pattern or arrangement. They also move at a constant speed and in a straight line, until they collide with other particles or the walls of the container. This assumption helps explain the macroscopic properties of gases, such as pressure and temperature, based on the behavior of individual gas particles.Rate this question:
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- 11.
Under which conditions of temperature and pressure would a sample of H2(g) behave most like an ideal gas?
- A.
0°C and 100 kPa
- B.
0°C and 300 kPa
- C.
150°C and 100 kPa
- D.
150°C and 300 kPa
Correct Answer
C. 150°C and 100 kPaExplanation
At higher temperatures and lower pressures, a gas is more likely to behave like an ideal gas. In this case, 150°C and 100 kPa represent higher temperature and lower pressure compared to the other options, making it the best choice for the sample of H2(g) to behave most like an ideal gas.Rate this question:
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- 12.
A real gas behaves least like an ideal gas under the conditions of
- A.
Low temperature and low pressure
- B.
Low temperature and high pressure
- C.
High temperature and low pressure
- D.
High temperature and high pressure
Correct Answer
C. High temperature and low pressureExplanation
At high temperature and low pressure, the intermolecular forces between the gas particles become significant and cannot be ignored. These forces cause the gas particles to deviate from ideal behavior, resulting in a decrease in the gas's resemblance to an ideal gas. As a result, the gas behaves least like an ideal gas under these conditions.Rate this question:
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Current Version
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Mar 21, 2023Quiz Edited by
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Dec 07, 2011Quiz Created by
Ionca
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