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According to the Kinetic Molecular Theory of Gases, increasing the temperature of a gas sample at constant volume will result in:
- a)An increase in the number of gas molecules.
- b)A decrease in the average kinetic energy of the gas molecules.
- c)An increase in the pressure of the gas.
- d)No change in the behavior of the gas.
Correct answer is option 'C'. Can you explain this answer?
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According to the Kinetic Molecular Theory of Gases, increasing the tem...
Understanding the Kinetic Molecular Theory of Gases
The Kinetic Molecular Theory (KMT) offers insights into the behavior of gases, particularly how temperature affects their characteristics.
Temperature and Kinetic Energy
- Kinetic Energy: According to KMT, the temperature of a gas is directly related to the average kinetic energy of its molecules.
- Effect of Temperature Increase: When the temperature of a gas increases, the average kinetic energy of the gas molecules also increases. This means that the molecules move faster.
Constant Volume Implications
- Constant Volume: If the gas is held at a constant volume, the space available for the gas molecules to move does not change.
- Resulting Pressure Increase: As the temperature rises, the faster-moving molecules collide with the walls of the container more frequently and with greater force.
Pressure Change in Gases
- Pressure and Temperature Relationship: At constant volume, increasing the temperature leads to an increase in pressure. This is described by the ideal gas law, where pressure is directly proportional to temperature (in Kelvin) when volume is constant.
Correct Answer Explanation
- Option C: Therefore, the correct answer to the question is option 'C' - an increase in the pressure of the gas.
- Other Options:
- Option 'A' is incorrect as the number of gas molecules remains constant.
- Option 'B' is incorrect since temperature increase raises the average kinetic energy, not decreases it.
- Option 'D' is also incorrect; the behavior of the gas changes with temperature.
In summary, increasing the temperature of a gas at constant volume results in increased pressure due to heightened molecular activity.
The Kinetic Molecular Theory (KMT) offers insights into the behavior of gases, particularly how temperature affects their characteristics.
Temperature and Kinetic Energy
- Kinetic Energy: According to KMT, the temperature of a gas is directly related to the average kinetic energy of its molecules.
- Effect of Temperature Increase: When the temperature of a gas increases, the average kinetic energy of the gas molecules also increases. This means that the molecules move faster.
Constant Volume Implications
- Constant Volume: If the gas is held at a constant volume, the space available for the gas molecules to move does not change.
- Resulting Pressure Increase: As the temperature rises, the faster-moving molecules collide with the walls of the container more frequently and with greater force.
Pressure Change in Gases
- Pressure and Temperature Relationship: At constant volume, increasing the temperature leads to an increase in pressure. This is described by the ideal gas law, where pressure is directly proportional to temperature (in Kelvin) when volume is constant.
Correct Answer Explanation
- Option C: Therefore, the correct answer to the question is option 'C' - an increase in the pressure of the gas.
- Other Options:
- Option 'A' is incorrect as the number of gas molecules remains constant.
- Option 'B' is incorrect since temperature increase raises the average kinetic energy, not decreases it.
- Option 'D' is also incorrect; the behavior of the gas changes with temperature.
In summary, increasing the temperature of a gas at constant volume results in increased pressure due to heightened molecular activity.
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According to the Kinetic Molecular Theory of Gases, increasing the tem...
According to the Kinetic Molecular Theory, increasing the temperature of a gas sample at constant volume will result in an increase in the average kinetic energy of the gas molecules, leading to more frequent and energetic collisions with the container walls, thus increasing the pressure.
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According to the Kinetic Molecular Theory of Gases, increasing the temperature of a gas sample at constant volume will result in:a)An increase in the number of gas molecules.b)A decrease in the average kinetic energy of the gas molecules.c)An increase in the pressure of the gas.d)No change in the behavior of the gas.Correct answer is option 'C'. Can you explain this answer?
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