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At constant volume, for a fixed number of moles of a gas, the pressure of the gas increases with an increase in temperature due to:
a) Increase in the average molecule speed
b) Increase in rate of collision amongst molecules
c) Increase in molecular attraction
d) Increase in mean free path
Correct answer is option 'A'. Can you explain this answer?
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At constant volume, for a fixed number of moles of a gas, the pressure...
Pressure on the walls of the container is equal to the change of momentum per unit time per unit area. At constant volume, for a fixed number of moles of a gas, the pressure increases with rise in temperature due to increase in average molecular speed. This increases the change in momentum during collisions.
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At constant volume, for a fixed number of moles of a gas, the pressure...
Explanation:
Under constant volume, the pressure of a gas is directly proportional to the temperature. The increase in temperature leads to an increase in the kinetic energy of the molecules of the gas, which in turn increases the pressure of the gas. This can be explained by the following reasons:
Increase in the average molecule speed:
When the temperature of a gas is increased, the average kinetic energy of its molecules also increases. The kinetic energy of a gas is related to the speed of its molecules. Therefore, an increase in temperature results in an increase in the average speed of the molecules. As the molecules move faster, they collide with each other and with the container walls more frequently, resulting in an increase in pressure. Therefore, option A is the correct answer.
Increase in rate of collision amongst molecules:
When the temperature of a gas is increased, the molecules of the gas move faster and collide more frequently with each other. This results in an increase in the rate of collision amongst the molecules. As a result, the pressure of the gas increases.
Increase in molecular attraction:
When the temperature of a gas is increased, the intermolecular attraction between the molecules decreases. This is because the increased kinetic energy of the molecules overcomes the attractive forces between them. Therefore, an increase in temperature would not lead to an increase in the pressure of the gas due to an increase in molecular attraction.
Increase in mean free path:
The mean free path is the average distance travelled by a molecule of a gas between collisions. When the temperature of a gas is increased, the mean free path of the molecules also increases. This is because the molecules move faster and collide less frequently. However, this increase in mean free path would not result in an increase in the pressure of the gas.
Under constant volume, the pressure of a gas is directly proportional to the temperature. The increase in temperature leads to an increase in the kinetic energy of the molecules of the gas, which in turn increases the pressure of the gas. This can be explained by the following reasons:
Increase in the average molecule speed:
When the temperature of a gas is increased, the average kinetic energy of its molecules also increases. The kinetic energy of a gas is related to the speed of its molecules. Therefore, an increase in temperature results in an increase in the average speed of the molecules. As the molecules move faster, they collide with each other and with the container walls more frequently, resulting in an increase in pressure. Therefore, option A is the correct answer.
Increase in rate of collision amongst molecules:
When the temperature of a gas is increased, the molecules of the gas move faster and collide more frequently with each other. This results in an increase in the rate of collision amongst the molecules. As a result, the pressure of the gas increases.
Increase in molecular attraction:
When the temperature of a gas is increased, the intermolecular attraction between the molecules decreases. This is because the increased kinetic energy of the molecules overcomes the attractive forces between them. Therefore, an increase in temperature would not lead to an increase in the pressure of the gas due to an increase in molecular attraction.
Increase in mean free path:
The mean free path is the average distance travelled by a molecule of a gas between collisions. When the temperature of a gas is increased, the mean free path of the molecules also increases. This is because the molecules move faster and collide less frequently. However, this increase in mean free path would not result in an increase in the pressure of the gas.
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At constant volume, for a fixed number of moles of a gas, the pressure...
Average speed = √(8RT/πM) ie, at constant volume, for a fixed mass, increasing temperature increases average speeds and molecules collide more frequently to the wall of container leading to increase in gas pressure.
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