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Why at extremely low pressures, the real gases obey the ideal gas equation? |
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Answer» At low pressures, volume V is very large and hence the correction term b (volume correction term) can be neglected in comparison to very large value of V. Thus, the van der Waals equation for 1 mole of a real gas. \(\big(p+\frac{a}{V^2}\big)(V-b)\)RT may be written as \(\big(p+\frac{a}{V^2}\big)(V)\) = RT Or PV + \(\frac{a}{V}\) = RT PV = RT - \(\frac{a}{V}\) For large V (at very low pressure),\(\frac{a}{V}\) is very small and can be ignored. \(\therefore\) PV becomes RT at very low pressure. That is why at very low pressure, real gases obey ideal gas equation. |
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