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At constant volume, temperature is increased then
- a)collision on walls will be less [1989]
- b)number of collisions per unit time will increase
- c)collisions will be in straight lines
- d)collisions will not change.
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
At constant volume, temperature is increased thena)collision on walls ...
As the temperature increases, the average velocity increases. So, the collisions are faster.
Most Upvoted Answer
At constant volume, temperature is increased thena)collision on walls ...
Explanation:
At constant volume, the pressure of a gas is directly proportional to its temperature. When the temperature of a gas at constant volume is increased, the gas molecules gain kinetic energy and move faster. This increase in kinetic energy leads to an increase in the number of collisions between gas molecules and the walls of the container.
Reasoning:
There are a few key points to consider when answering this question:
1. Collision frequency: The frequency of collisions between gas molecules and the walls of the container is determined by the speed and number of gas molecules. As the temperature is increased, the average speed of the gas molecules increases, leading to an increase in the number of collisions per unit time.
2. Collision probability: The probability of a collision occurring depends on the straight-line path followed by the gas molecules. At higher temperatures, the gas molecules move with increased speed and are more likely to move in straight lines, resulting in a higher probability of collisions with the walls of the container.
3. Pressure: The pressure exerted by a gas is directly related to the number of collisions per unit time and the force exerted by each collision. As the number of collisions increases, the pressure of the gas also increases.
Conclusion:
Based on the above reasoning, it can be concluded that at constant volume, an increase in temperature will lead to an increase in the number of collisions per unit time between gas molecules and the walls of the container. Therefore, option B is the correct answer.
At constant volume, the pressure of a gas is directly proportional to its temperature. When the temperature of a gas at constant volume is increased, the gas molecules gain kinetic energy and move faster. This increase in kinetic energy leads to an increase in the number of collisions between gas molecules and the walls of the container.
Reasoning:
There are a few key points to consider when answering this question:
1. Collision frequency: The frequency of collisions between gas molecules and the walls of the container is determined by the speed and number of gas molecules. As the temperature is increased, the average speed of the gas molecules increases, leading to an increase in the number of collisions per unit time.
2. Collision probability: The probability of a collision occurring depends on the straight-line path followed by the gas molecules. At higher temperatures, the gas molecules move with increased speed and are more likely to move in straight lines, resulting in a higher probability of collisions with the walls of the container.
3. Pressure: The pressure exerted by a gas is directly related to the number of collisions per unit time and the force exerted by each collision. As the number of collisions increases, the pressure of the gas also increases.
Conclusion:
Based on the above reasoning, it can be concluded that at constant volume, an increase in temperature will lead to an increase in the number of collisions per unit time between gas molecules and the walls of the container. Therefore, option B is the correct answer.
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At constant volume, temperature is increased thena)collision on walls will be less [1989]b)number of collisions per unit time will increasec)collisions will be in straight linesd)collisions will not change.Correct answer is option 'B'. Can you explain this answer?
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