Gases & Solutions
States of Matter
Why at extremely low pressures, the real gases obey the ideal gas equation?
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
For large (at very low pressures) is very small and can be ignored.
becomes at very low pressures.