Q. According to the kinetic theory, what happens to the pressure of a gas if the temperature is doubled while keeping the volume constant?
A.
Pressure remains the same
B.
Pressure doubles
C.
Pressure triples
D.
Pressure halves
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Solution
According to the ideal gas law, if temperature is doubled and volume is constant, pressure also doubles.
Correct Answer:
B
— Pressure doubles
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Q. In an ideal gas, what is the relationship between the average kinetic energy and the absolute temperature?
A.
Directly proportional
B.
Inversely proportional
C.
No relationship
D.
Exponential relationship
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Solution
The average kinetic energy of gas molecules is directly proportional to the absolute temperature.
Correct Answer:
A
— Directly proportional
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Q. In the kinetic theory of gases, which of the following assumptions is NOT true?
A.
Gas molecules are in constant random motion
B.
Gas molecules occupy a negligible volume
C.
Gas molecules experience no intermolecular forces
D.
Gas molecules have significant mass
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Solution
In the kinetic theory of gases, it is assumed that gas molecules occupy a negligible volume and have negligible mass compared to the volume they occupy.
Correct Answer:
D
— Gas molecules have significant mass
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Q. In the kinetic theory, what is assumed about the collisions between gas molecules?
A.
They are perfectly elastic
B.
They are perfectly inelastic
C.
They lose energy
D.
They are not considered
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Solution
In the kinetic theory of gases, it is assumed that collisions between gas molecules are perfectly elastic, meaning they conserve kinetic energy.
Correct Answer:
A
— They are perfectly elastic
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Q. What does the term 'mean free path' refer to in the context of gases?
A.
The average distance traveled by a molecule between collisions
B.
The average speed of gas molecules
C.
The average time between collisions
D.
The average kinetic energy of gas molecules
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Solution
The mean free path is defined as the average distance a molecule travels before colliding with another molecule.
Correct Answer:
A
— The average distance traveled by a molecule between collisions
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Q. What is the effect of increasing the temperature of a gas on its average molecular speed?
A.
Average speed decreases
B.
Average speed remains the same
C.
Average speed increases
D.
Average speed becomes zero
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Solution
Increasing the temperature of a gas increases the average kinetic energy of its molecules, which in turn increases their average speed.
Correct Answer:
C
— Average speed increases
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Q. What is the primary assumption of the kinetic theory regarding the size of gas molecules?
A.
Gas molecules are very large
B.
Gas molecules are very small
C.
Gas molecules have significant volume
D.
Gas molecules are incompressible
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Solution
The kinetic theory assumes that gas molecules are very small compared to the distances between them, allowing for negligible volume.
Correct Answer:
B
— Gas molecules are very small
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Q. What is the primary reason gases expand to fill their containers?
A.
Molecules are attracted to the walls
B.
Molecules are in constant random motion
C.
Molecules have high mass
D.
Molecules are inelastic
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Solution
Gases expand to fill their containers because their molecules are in constant random motion, colliding with the walls of the container.
Correct Answer:
B
— Molecules are in constant random motion
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Q. What is the relationship between the root mean square speed (v_rms) and temperature (T) for an ideal gas?
A.
v_rms = sqrt(3kT/m)
B.
v_rms = sqrt(2kT/m)
C.
v_rms = sqrt(kT/m)
D.
v_rms = 3kT/m
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Solution
The root mean square speed is given by v_rms = sqrt(3kT/m), where k is the Boltzmann constant and m is the mass of a gas molecule.
Correct Answer:
A
— v_rms = sqrt(3kT/m)
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Q. Which of the following factors does NOT affect the pressure of an ideal gas?
A.
Temperature
B.
Volume
C.
Number of molecules
D.
Color of the gas
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Solution
The pressure of an ideal gas is affected by temperature, volume, and the number of molecules, but not by the color of the gas.
Correct Answer:
D
— Color of the gas
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