A gas described by van der Waal's equation: | vedclass

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(A) The van der Waal's equation is given by $\left(P + \frac{n^2 a}{V^2}ight)(V - nb) = nRT$.$A$. At large molar volumes $(V 	o \infty)$,the terms

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$A, C, D$

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(A) The van der Waal's equation is given by $\left(P + \frac{n^2 a}{V^2}ight)(V - nb) = nRT$.$A$. At large molar volumes $(V 	o \infty)$,the terms $\frac{n^2 a}{V^2}$ and $nb$ become negligible,so the equation reduces to $PV = nRT$,behaving like an ideal gas. This is correct.$B$. At large pressures,the volume $V$ is small,and the correction terms become significant,so it deviates from ideal behavior. This is incorrect.$C$. The constants $a$ (intermolecular forces) and $b$ (excluded volume) are characteristic of the specific gas and are independent of temperature. This is correct.$D$. Since $P = \frac{nRT}{V-nb} - \frac{n^2 a}{V^2}$,the pressure $P$ of a real gas is lower than the ideal pressure $P_{ideal} = \frac{nRT}{V}$ due to the attractive force term $\frac{n^2 a}{V^2}$. This is correct.

$A$ gas described by van der Waal's equation:

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