Why at extremely low pressures, the real gases obey the ideal gas | Filo
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Class 11

Chemistry

Gases & Solutions

States of Matter

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Why at extremely low pressures, the real gases obey the ideal gas equation?

Solution:
At low pressures, volume is very large and hence the correction term b (a constant of small value) can be neglected in comparison to the very large value of . Thus the van der Waal's equation for mole of a real gas. 

may be written as

or

or

For large (at very low pressures) is very small and can be ignored.

becomes at very low pressures.
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