(B) For an ideal gas,$PV = nRT$. Given $n = 1 \, mol$,$V = 22.4 \, L$,and $T = 273 \, K$,the ideal pressure $P_{ideal} = \frac{nRT}{V} = \frac{1 \time

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If compressibility factor $(Z) > 1$,then $P$ will be greater than $1 \, atm$.

(B) For an ideal gas,$PV = nRT$. Given $n = 1 \, mol$,$V = 22.4 \, L$,and $T = 273 \, K$,the ideal pressure $P_{ideal} = \frac{nRT}{V} = \frac{1 \times 0.0821 \times 273}{22.4} \approx 1 \, atm$.By definition,the compressibility factor is $Z = \frac{PV}{nRT}$.Therefore,$P = \frac{Z \times nRT}{V} = Z \times P_{ideal}$.If $Z > 1$,then $P > P_{ideal}$,which means $P > 1 \, atm$.

Class 11 Chemistry States of Matter Real gases and Vander waal’s equation

Medium

The correct option regarding a container containing $1 \, mol$ of a gas in a $22.4 \, L$ container at $273 \, K$ is:

A
If compressibility factor $(Z) > 1$,then $P$ will be less than $1 \, atm$.
B
If compressibility factor $(Z) > 1$,then $P$ will be greater than $1 \, atm$.
C
If $b$ dominates,pressure will be less than $1 \, atm$.
D
If $a$ dominates,pressure will be greater than $1 \, atm$.

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Real gases and Vander waal’s equation

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In the van der Waals equation for gases,what does the constant $b$ represent?

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The correct option regarding a container containing $1 \, mol$ of a gas in a $22.4 \, L$ container at $273 \, K$ is:

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What is the volume of $1 \ mole$ of a real gas at $STP$ $(V_{ideal} = 22.4 \ dm^3)$,if the compressibility factor of the real gas is $1.1$ at $STP$ (in $dm^3$)?

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