Why are real gases different from ideal gases, and how does kinetic theory address this?
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1 Answer
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The main difference between the real and ideal gases is with respect to the kinetic theory. The ideal gas follows assumptions of the kinetic theory but the real gases do not follow it, especially when the temperature is low and there is high pressure.
The following points are applicable in the case of real gases:
- Real gas molecules do have finite volume.
- In such cases, intermolecular forces such as Van there Waals forces become significant.
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4.22

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So the magnitude of vector + =
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Let = -
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Hence = . Therefore the magnitude of ( + =
Let
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