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The pressure of a given mass of gas, held at constant volume, is directly proportional to its absolute temperature. This may be stated mathematically as:
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| i = initial state of process |
| f = final state of process |
For example if we take a sealed container of gas and double its absolute temperature its pressure will double.
This reason for the increase in pressure is that the heated molecules vibrate faster and therefore have more kinetic energy. Within a fixed volume they will collide with the container walls with greater force. The increase in force is felt as an increase in pressure.
The simple experiment below will demonstrate this relationship by allowing you to vary the temperature of a gas and observe the effect on its pressure.
Click on the button to vary the temperature
We have now examined the relationships of volume to pressure, volume to temperature and pressure to temperature of a gas. The next page will look at equation which combines these relationships. This is known as:
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| Volume and Temperature | The Atmosphere | The Ideal Gas Law | |||