CBSE Class 11-science Answered
How to prove the conditions for a real gas to be ideal?
Asked by tinku4121999 | 17 Sep, 2015, 08:03: PM
Expert Answer
- Gases show deviation from ideal behaviour because of two faulty assumptions:
- There is no force of attraction between the molecules of a gas.
- Volume of the molecules of a gas is negligibly small in comparison to the space occupied by the gas.
- At low temperature and high pressure, gases deviate from ideal behaviour, i.e. gases behave as real gases.
- At low pressure and high temperature gases show ideal behaviour, i.e. gases behave as ideal gases.
- Plot of pressure–volume (pV) versus pressure (p) at constant temperature for ideal and real gases.
- Plot of pressure (p) versus volume (V) for ideal and real gases.
- Van der Waals equation of state is given below:
- The deviation from ideal behaviour can be measured in terms of the compressibility factor Z, which is the ratio of product pV and nRT.
- The deviations from ideal behavior become less and less with increase in temperature.
- The temperature at which a real gas obeys ideal gas law over an appreciable range of pressure is called Boyle temperature or Boyle point.
Answered by Prachi Sawant | 18 Sep, 2015, 09:27: AM
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