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Why at low pressures, the real gas behaves as ideal gas? |
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Answer» Solution :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 is nothing but representing the LIMITING behaviour of gases at infinite small pressures. |
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