A gas that follows Boyle's law,Charle's law a | vedclass

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(B) real gas behaves like an ideal gas when the intermolecular forces of attraction are negligible and the volume occupied by the gas molecules is neg

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Low pressure and high temperature

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(B) real gas behaves like an ideal gas when the intermolecular forces of attraction are negligible and the volume occupied by the gas molecules is negligible compared to the total volume of the gas. These conditions are achieved at $Low \ Pressure$ and $High \ Temperature$. At $Low \ Pressure$,the molecules are far apart,reducing intermolecular interactions. At $High \ Temperature$,the kinetic energy of the molecules is high,which overcomes the intermolecular forces of attraction.

$A$ gas that follows Boyle's law,Charle's law and Avogadro's law is called an ideal gas. Under what conditions does a real gas behave ideally?

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For real gases,the relation between $P$,$V$ and $T$ is given by the van der Waals equation,$(P + \frac{an^2}{V^2})(V - nb) = nRT$. For the following gases $CH_4, CO_2, O_2, H_2$,which gas will have $(i)$ highest value of $'a'$ $(ii)$ lowest value of $'b'$?

If $Z$ is a compressibility factor,the van der Waals equation at low pressure can be written as:

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