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The temperature of a gas is raised while its volume remains constant, the pressure exerted by a gas on the walls of the container increases because its molecules.
Select one:
Select one:
- a)collide with each other less frequently
- b)strike the wall more often with higher velocities
- c)lose more kinetic energy to the wall
- d)are in contact with the wall for a shorter time
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
The temperature of a gas is raised while its volume remains constant, ...
Due to increase in temperature, root mean square velocity of gas molecule increases. So they strike the wall more often with higher velocity. Hence, the pressure exerted by a gas on the walls of the container increases.
The correct answer is: strike the wall more often with higher velocities
The correct answer is: strike the wall more often with higher velocities
Most Upvoted Answer
The temperature of a gas is raised while its volume remains constant, ...
Explanation:
Pressure is defined as the force exerted per unit area by the molecules of a gas on the walls of the container. When the temperature of a gas is raised while its volume remains constant, the average kinetic energy of the gas molecules increases. This increase in kinetic energy leads to an increase in the speed of the gas molecules.
Reasoning:
- Higher Velocities: When the temperature is increased, the gas molecules move faster and collide with the walls of the container more frequently. These collisions with higher velocities result in a greater force being exerted on the walls of the container, leading to an increase in pressure.
- More Frequent Collisions: The increased speed of the gas molecules also means that they strike the walls of the container more often, further contributing to the increase in pressure.
- Constant Volume: Since the volume of the gas remains constant in this scenario, the gas molecules do not have more space to occupy. Therefore, the increase in kinetic energy due to the temperature rise is manifested as an increase in pressure on the walls of the container.
In conclusion, when the temperature of a gas is raised while its volume remains constant, the pressure exerted by the gas on the walls of the container increases because the gas molecules strike the wall more often with higher velocities.
Pressure is defined as the force exerted per unit area by the molecules of a gas on the walls of the container. When the temperature of a gas is raised while its volume remains constant, the average kinetic energy of the gas molecules increases. This increase in kinetic energy leads to an increase in the speed of the gas molecules.
Reasoning:
- Higher Velocities: When the temperature is increased, the gas molecules move faster and collide with the walls of the container more frequently. These collisions with higher velocities result in a greater force being exerted on the walls of the container, leading to an increase in pressure.
- More Frequent Collisions: The increased speed of the gas molecules also means that they strike the walls of the container more often, further contributing to the increase in pressure.
- Constant Volume: Since the volume of the gas remains constant in this scenario, the gas molecules do not have more space to occupy. Therefore, the increase in kinetic energy due to the temperature rise is manifested as an increase in pressure on the walls of the container.
In conclusion, when the temperature of a gas is raised while its volume remains constant, the pressure exerted by the gas on the walls of the container increases because the gas molecules strike the wall more often with higher velocities.
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The temperature of a gas is raised while its volume remains constant, the pressure exerted by a gas on the walls of the container increases because its molecules.Select one:a)collide with each other less frequentlyb)strike the wall more often with higher velocitiesc)lose more kinetic energy to the walld)are in contact with the wall for a shorter timeCorrect answer is option 'B'. Can you explain this answer?
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