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

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

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

Vedclass · Accepted Answer

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

Vedclass · Answer

(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

If $Z$ is the compressibility factor,then for $1 \, \text{mole}$ of a real gas,the van der Waals equation at low pressure can be written as:

Real gases show deviation from ideal behavior. Explain with examples.

Explain: Why do real gases show deviation from ideal gas behavior?

"Real gases do not follow Boyle's Law,Charles's Law,and Avogadro's Law perfectly under all conditions." Explain.

The compressibility factor for a real gas at high pressure is :-

Vedclass Test Series

Exam Paper Generator

Online Exam Module