The compressibility factor (z) is lower for N | vedclass

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(A) The compressibility factor $(z)$ is defined as $z = PV/nRT$. For real gases, the deviation from ideal behavior is primarily due to intermolecular

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van der Waals constants $'a'$ of $CO_2$ and $NH_3$ are greater than that of $N_2$

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(A) The compressibility factor $(z)$ is defined as $z = PV/nRT$. For real gases, the deviation from ideal behavior is primarily due to intermolecular forces of attraction, represented by the van der Waals constant $'a'$. $A$ higher value of $'a'$ indicates stronger intermolecular forces of attraction. Stronger attractive forces lead to a greater negative deviation from ideal behavior, resulting in a lower compressibility factor $(z Since $NH_3$ and $CO_2$ are polar or more easily liquefiable than $N_2$, they have larger values of the constant $'a'$ compared to $N_2$. Therefore, the compressibility factor is lower for $NH_3$ and $CO_2$ than for $N_2$.

The compressibility factor $(z)$ is lower for $NH_3$ and $CO_2$ gases than that of $N_2$ gas, because

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