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(A) The Van der Waals equation for $n$ moles of a real gas is given by: $(P + \frac{an^2}{V^2})(V - nb) = nRT$. For a real gas to behave like an ideal

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constants $a$ and $b$ are small

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(A) The Van der Waals equation for $n$ moles of a real gas is given by: $(P + \frac{an^2}{V^2})(V - nb) = nRT$. For a real gas to behave like an ideal gas,the deviations from ideal behavior must be minimized. $1$. The term $\frac{an^2}{V^2}$ accounts for intermolecular forces of attraction. If $a$ is small,these forces are negligible. $2$. The term $nb$ accounts for the finite volume occupied by gas molecules. If $b$ is small,the volume of the molecules is negligible compared to the total volume of the container. Therefore,when both Van der Waals constants $a$ and $b$ are small,the real gas equation reduces to the ideal gas equation $PV = nRT$.

$A$ real gas obeying Van der Waals equation will resemble an ideal gas if the:

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