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

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Question

(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

Similar Questions

Assertion : Compressibility factor $(Z)$ for non-ideal gases can be greater than $1$.
Reason : Non-ideal gases always exert higher pressure than expected.

In Van der Waals equation of state for a non-ideal gas,the term that accounts for intermolecular forces is

The correction factor '$a$' in the van der Waals equation for real gases corresponds to:

$A$ gas deviates most from ideal behavior when it is subjected to

Under which conditions will a real gas behave most like an ideal gas?

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