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All questions of Kinetic Molecular Theory of Gases for MCAT Exam
Which of the following assumptions is NOT part of the Kinetic Molecular Theory of Gases?- a)Gas molecules occupy a negligible volume.
- b)Gas molecules are in constant motion.
- c)Gas molecules have strong attractive forces between them.
- d)Gas molecules undergo elastic collisions.
Correct answer is option 'C'. Can you explain this answer?
Which of the following assumptions is NOT part of the Kinetic Molecular Theory of Gases?
a)
Gas molecules occupy a negligible volume.
b)
Gas molecules are in constant motion.
c)
Gas molecules have strong attractive forces between them.
d)
Gas molecules undergo elastic collisions.
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Ayesha Joshi answered |
The Kinetic Molecular Theory assumes that gas molecules do not have strong attractive forces between them. Instead, they only interact through collisions.
According to the Kinetic Molecular Theory of Gases, increasing the temperature of a gas sample at constant volume will result in:- a)An increase in the number of gas molecules.
- b)A decrease in the average kinetic energy of the gas molecules.
- c)An increase in the pressure of the gas.
- d)No change in the behavior of the gas.
Correct answer is option 'C'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, increasing the temperature of a gas sample at constant volume will result in:
a)
An increase in the number of gas molecules.
b)
A decrease in the average kinetic energy of the gas molecules.
c)
An increase in the pressure of the gas.
d)
No change in the behavior of the gas.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, increasing the temperature of a gas sample at constant volume will result in an increase in the average kinetic energy of the gas molecules, leading to more frequent and energetic collisions with the container walls, thus increasing the pressure.
According to the Kinetic Molecular Theory of Gases, which of the following statements about the volume of gas molecules is true?- a)Gas molecules have a significant volume compared to the volume of the container.
- b)Gas molecules have a negligible volume compared to the volume of the container.
- c)The volume of gas molecules is inversely proportional to the pressure of the gas.
- d)The volume of gas molecules is directly proportional to the temperature of the gas.
Correct answer is option 'B'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, which of the following statements about the volume of gas molecules is true?
a)
Gas molecules have a significant volume compared to the volume of the container.
b)
Gas molecules have a negligible volume compared to the volume of the container.
c)
The volume of gas molecules is inversely proportional to the pressure of the gas.
d)
The volume of gas molecules is directly proportional to the temperature of the gas.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, gas molecules are assumed to have a negligible volume compared to the volume of the container. This assumption allows us to treat gases as point particles.
According to the Kinetic Molecular Theory of Gases, the pressure exerted by a gas is due to:- a)The total mass of the gas molecules.
- b)The volume occupied by the gas.
- c)The average kinetic energy of the gas molecules.
- d)The number of gas molecules present.
Correct answer is option 'C'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, the pressure exerted by a gas is due to:
a)
The total mass of the gas molecules.
b)
The volume occupied by the gas.
c)
The average kinetic energy of the gas molecules.
d)
The number of gas molecules present.
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Ayesha Joshi answered |
The pressure exerted by a gas is a result of the collisions between gas molecules and the walls of the container. According to the Kinetic Molecular Theory, the average kinetic energy of the gas molecules determines the magnitude of these collisions and thus the pressure.
According to the Kinetic Molecular Theory of Gases, what happens to the average kinetic energy of gas molecules when the temperature is doubled?- a)It is halved.
- b)It is quadrupled.
- c)It remains the same.
- d)It cannot be determined without more information.
Correct answer is option 'B'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, what happens to the average kinetic energy of gas molecules when the temperature is doubled?
a)
It is halved.
b)
It is quadrupled.
c)
It remains the same.
d)
It cannot be determined without more information.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, the average kinetic energy of gas molecules is directly proportional to the temperature. Therefore, doubling the temperature will result in quadrupling the average kinetic energy.
According to the Kinetic Molecular Theory of Gases, which of the following statements is true?- a)Gas molecules have no mass.
- b)Gas molecules are in constant random motion.
- c)Gas molecules always occupy the entire volume of their container.
- d)Gas molecules only interact with each other through chemical reactions.
Correct answer is option 'B'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, which of the following statements is true?
a)
Gas molecules have no mass.
b)
Gas molecules are in constant random motion.
c)
Gas molecules always occupy the entire volume of their container.
d)
Gas molecules only interact with each other through chemical reactions.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, gas molecules are in constant motion, moving in random directions and colliding with each other and the walls of the container.
According to the Kinetic Molecular Theory of Gases, how do the average velocities of gas molecules compare at the same temperature, but with different molar masses?- a)The average velocities are the same.
- b)The average velocities are directly proportional to the molar masses.
- c)The average velocities are inversely proportional to the molar masses.
- d)The average velocities cannot be determined without more information.
Correct answer is option 'C'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, how do the average velocities of gas molecules compare at the same temperature, but with different molar masses?
a)
The average velocities are the same.
b)
The average velocities are directly proportional to the molar masses.
c)
The average velocities are inversely proportional to the molar masses.
d)
The average velocities cannot be determined without more information.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, at the same temperature, gas molecules with higher molar masses will have lower average velocities. This is because the kinetic energy is the same for all gas molecules at a given temperature, but lighter molecules will have higher speeds to compensate for their lower mass, while heavier molecules will have lower speeds.
According to the Kinetic Molecular Theory of Gases, under what conditions will a gas behave most ideally?- a)Low pressure and high temperature
- b)High pressure and low temperature
- c)High pressure and high temperature
- d)Low pressure and low temperature
Correct answer is option 'A'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, under what conditions will a gas behave most ideally?
a)
Low pressure and high temperature
b)
High pressure and low temperature
c)
High pressure and high temperature
d)
Low pressure and low temperature
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, a gas behaves most ideally under conditions of low pressure and high temperature. At low pressures, gas molecules are far apart and experience fewer intermolecular forces. At high temperatures, gas molecules have higher kinetic energy and move more rapidly, reducing the effect of intermolecular forces.
Which of the following statements is consistent with the Kinetic Molecular Theory of Gases?- a)The pressure of a gas decreases with an increase in temperature.
- b)The volume of a gas decreases with an increase in pressure.
- c)The speed of gas molecules decreases with a decrease in temperature.
- d)The density of a gas decreases with an increase in volume.
Correct answer is option 'C'. Can you explain this answer?
Which of the following statements is consistent with the Kinetic Molecular Theory of Gases?
a)
The pressure of a gas decreases with an increase in temperature.
b)
The volume of a gas decreases with an increase in pressure.
c)
The speed of gas molecules decreases with a decrease in temperature.
d)
The density of a gas decreases with an increase in volume.
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Ayesha Joshi answered |
According to the Kinetic Molecular Theory, the average speed of gas molecules is directly proportional to the temperature. Therefore, as the temperature decreases, the speed of gas molecules also decreases.
According to the Kinetic Molecular Theory of Gases, which of the following variables is directly proportional to the average kinetic energy of gas molecules?- a)Temperature
- b)Pressure
- c)Volume
- d)Mass
Correct answer is option 'A'. Can you explain this answer?
According to the Kinetic Molecular Theory of Gases, which of the following variables is directly proportional to the average kinetic energy of gas molecules?
a)
Temperature
b)
Pressure
c)
Volume
d)
Mass
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Ayesha Joshi answered |
The average kinetic energy of gas molecules is directly proportional to the temperature of the gas, according to the Kinetic Molecular Theory.
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