Explain the effect of high pressure and low t | vedclass

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(B) Boyle's law states that for a fixed amount of an ideal gas at constant temperature,the pressure is inversely proportional to its volume $(P \propt

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Boyle's law shows significant deviations.

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(B) Boyle's law states that for a fixed amount of an ideal gas at constant temperature,the pressure is inversely proportional to its volume $(P \propto \frac{1}{V})$.High Pressure: At high pressure,the intermolecular forces of attraction become significant,and the volume of gas molecules is no longer negligible compared to the total volume. Consequently,real gases deviate from ideal behavior,and the $P$ vs $\frac{1}{V}$ plot is not a straight line.Low Temperature: At low temperatures,the kinetic energy of gas molecules decreases,making intermolecular forces more effective. This causes the gas to deviate from ideal behavior,and Boyle's law is not followed strictly.

Gas	$a / (kPa \cdot dm^6 \cdot mol^{-2})$	$b / (dm^3 \cdot mol^{-1})$
$A$	$642.32$	$0.05196$
$B$	$155.21$	$0.04136$
$C$	$431.91$	$0.05196$
$D$	$155.21$	$0.4382$

Explain the effect of high pressure and low temperature on the validity of Boyle's law.

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Explain real gases showing deviations from ideal gas with correction of pressure and volume and derive van der Waals equation.

Consider the following table:

Gas $a / (kPa \cdot dm^6 \cdot mol^{-2})$ $b / (dm^3 \cdot mol^{-1})$

$A$ $642.32$ $0.05196$

$B$ $155.21$ $0.04136$

$C$ $431.91$ $0.05196$

$D$ $155.21$ $0.4382$

$a$ and $b$ are van der Waals constants. The correct statement about the gases is:

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