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(C) According to the kinetic molecular theory of gases,the assumptions that the volume of gas molecules is negligible compared to the total volume of

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high temperature and low pressure

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(C) According to the kinetic molecular theory of gases,the assumptions that the volume of gas molecules is negligible compared to the total volume of the gas and that there are no intermolecular forces of attraction are valid for an ideal gas.These conditions are best approximated by real gases at $high \ temperature$ and $low \ pressure$.At $high \ temperature$,the kinetic energy of the molecules is high,which overcomes the intermolecular forces of attraction.At $low \ pressure$,the molecules are far apart,making the volume occupied by the molecules themselves negligible compared to the total volume of the container.

List-$I$	List-$II$
$(1)$ Boyle's Law	$(A)$ $p \propto T$
$(2)$ Charles's Law	$(B)$ $V \propto n$
$(3)$ Gay-Lussac's Law	$(C)$ $p \propto \frac{1}{V}$
$(4)$ Avogadro's Law	$(D)$ $pV = nRT$
$(5)$ Ideal Gas Equation	$(E)$ $V = k_2T$

Molecular attraction and size of the molecules in a gas are negligible at :-

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