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According to kinetic theory of gases, for a diatomic molecule:
- a)The pressure exerted by the gas is proportional to the mean velocity of the molecule
- b)The pressure exerted by the gas is proportional to the root mean square velocity of the molecule
- c)The mean translational kinetic energy of the molecule is proportional to the absolute temperature
- d)The root mean square velocity of the molecule is inversely proportional to the temperature
Correct answer is option 'C'. Can you explain this answer?
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According to kinetic theory of gases, for a diatomic molecule:a)The pr...
According to the kinetic molecular theory, the average kinetic energy of gas particles is proportional to the absolute temperature of the gas. This can be expressed with the following equation where k represents the Boltzmann constant.
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According to kinetic theory of gases, for a diatomic molecule:a)The pr...
Kinetic Theory of Gases for Diatomic Molecules
Mean Translational Kinetic Energy is Proportional to Absolute Temperature
According to the kinetic theory of gases, the mean translational kinetic energy of a diatomic molecule is proportional to the absolute temperature. This means that as the temperature of the gas increases, the average kinetic energy of the molecules also increases. This is because at higher temperatures, the molecules have more kinetic energy and move faster.
Root Mean Square Velocity is Inversely Proportional to Temperature
The root mean square velocity of a diatomic molecule is inversely proportional to the temperature. This means that as the temperature of the gas increases, the root mean square velocity of the molecules decreases. This is because at higher temperatures, the molecules move faster, but the distribution of velocities becomes broader, with more molecules having velocities at the high end of the distribution and fewer at the low end.
Pressure is Proportional to Mean Velocity or Root Mean Square Velocity?
Neither the mean velocity nor the root mean square velocity of a diatomic molecule is directly proportional to the pressure exerted by the gas. Instead, the pressure is related to the total kinetic energy of the molecules, which is proportional to both the mean velocity and the root mean square velocity.
Conclusion
In conclusion, the kinetic theory of gases for diatomic molecules states that the mean translational kinetic energy of the molecules is proportional to the absolute temperature, and the root mean square velocity of the molecules is inversely proportional to the temperature. While neither of these directly relates to the pressure exerted by the gas, the pressure is related to the total kinetic energy of the molecules, which is proportional to both the mean velocity and the root mean square velocity.
Mean Translational Kinetic Energy is Proportional to Absolute Temperature
According to the kinetic theory of gases, the mean translational kinetic energy of a diatomic molecule is proportional to the absolute temperature. This means that as the temperature of the gas increases, the average kinetic energy of the molecules also increases. This is because at higher temperatures, the molecules have more kinetic energy and move faster.
Root Mean Square Velocity is Inversely Proportional to Temperature
The root mean square velocity of a diatomic molecule is inversely proportional to the temperature. This means that as the temperature of the gas increases, the root mean square velocity of the molecules decreases. This is because at higher temperatures, the molecules move faster, but the distribution of velocities becomes broader, with more molecules having velocities at the high end of the distribution and fewer at the low end.
Pressure is Proportional to Mean Velocity or Root Mean Square Velocity?
Neither the mean velocity nor the root mean square velocity of a diatomic molecule is directly proportional to the pressure exerted by the gas. Instead, the pressure is related to the total kinetic energy of the molecules, which is proportional to both the mean velocity and the root mean square velocity.
Conclusion
In conclusion, the kinetic theory of gases for diatomic molecules states that the mean translational kinetic energy of the molecules is proportional to the absolute temperature, and the root mean square velocity of the molecules is inversely proportional to the temperature. While neither of these directly relates to the pressure exerted by the gas, the pressure is related to the total kinetic energy of the molecules, which is proportional to both the mean velocity and the root mean square velocity.
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According to kinetic theory of gases, for a diatomic molecule:a)The pressure exerted by the gas is proportional to the mean velocity of the moleculeb)The pressure exerted by the gas is proportional to the root mean square velocity of the moleculec)The mean translational kinetic energy of the molecule is proportional to the absolute temperatured)The root mean square velocity of the molecule is inversely proportional to the temperatureCorrect answer is option 'C'. Can you explain this answer?
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