Assertion : Greater the value of van der Waal | vedclass

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(A) The van der Waal's constant $a$ represents the magnitude of intermolecular attractive forces in a gas. Higher values of $a$ indicate stronger attr

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If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

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(A) The van der Waal's constant $a$ represents the magnitude of intermolecular attractive forces in a gas. Higher values of $a$ indicate stronger attractive forces between gas molecules,which makes it easier for the gas to be liquefied. In the van der Waal's equation,the pressure correction term is $\frac{an^2}{V^2}$,where $a$ accounts for these attractive forces. Therefore,both the assertion and the reason are correct,and the reason is the correct explanation of the assertion.

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

Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.

Similar Questions

What are the corrections made to the pressure and volume of real gases compared to ideal gases?

The compressibility factor for a van der Waal gas at high pressure is

The van der Waals equation for $CH_4$ at low pressure is:

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:

For which of the following gases is the value of the van der Waals constant $'a'$ expected to be the highest?

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Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas. Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.