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Why at low pressures, the real gas behav...

Why at low pressures, the real gas behaves as ideal gas?

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At low pressures, when volume is large, both correction factors in the van der Waals. equations may be neglected.
The equation `(P + a/(V^2)) (V- b) = RT`, reduces to PV = RT, ideal gas law. This represents the limiting behaviour of gases at infinite small pressures .
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