The figure represents PV vs P relation for CO | vedclass

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

Question

(A) For real gases, the deviation from ideal behavior is described by the compressibility factor $Z = PV/nRT$. For gases with weak intermolecular forc

Vedclass · Accepted Answer

$1$

Vedclass · Answer

(A) For real gases, the deviation from ideal behavior is described by the compressibility factor $Z = PV/nRT$. For gases with weak intermolecular forces like $H_2$ and $He$, the repulsive forces dominate even at low pressures, causing $PV$ to increase continuously with pressure. Among $H_2$ and $He$, $He$ has weaker intermolecular forces and a smaller molecular size, leading to a steeper slope in the $PV$ vs $P$ plot. In the given graph, curves $1$ and $2$ show a continuous increase in $PV$ with $P$. Curve $1$ has a steeper slope than curve $2$. Therefore, curve $1$ represents $He$ and curve $2$ represents $H_2$.

The figure represents $PV$ vs $P$ relation for $CO$, $CH_4$, $H_2$ and $He$ gases under identical conditions. Which curve, shown in the figure, represents $He$ gas?

Similar Questions

At low pressure,the Van der Waals equation is reduced to:

When is deviation more in the behaviour of a gas from the ideal gas equation $PV = nRT$?

For one mole of a van der Waals gas when $b=0$ and $T=300 \ K$,the $PV$ vs. $1/V$ plot is shown below. The value of the van der Waals constant $a$ (in $\text{atm} \cdot \text{liter}^2 \cdot \text{mol}^{-2}$) is:

Excluded volume $(v)$ per molecule is related to the van der Waals constant $'b'$ in the following way:

Helium is suitable for gas thermometry at low temperatures because of its ...

Vedclass Test Series

Exam Paper Generator

Online Exam Module