The pressure of a real gas is less than the p | vedclass

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(D) In an ideal gas,it is assumed that there are no intermolecular forces of attraction between the gas molecules.However,in real gases,there exist in

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Intermolecular forces of attraction.

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(D) In an ideal gas,it is assumed that there are no intermolecular forces of attraction between the gas molecules.However,in real gases,there exist intermolecular forces of attraction.When a molecule approaches the wall of the container to exert pressure,it is pulled back by the other molecules in the bulk due to these attractive forces.As a result,the molecule hits the wall with less force than it would have in the absence of these attractions.Therefore,the observed pressure of a real gas is lower than the pressure of an ideal gas.

Gas	$a$ value
$1. C_6H_{6(g)}$	$a. 0.217$
$2. C_6H_5CH_{3(g)}$	$b. 5.464$
$3. Ne_{(g)}$	$c. 18.000$
$4. H_2O_{(g)}$	$d. 24.060$

The pressure of a real gas is less than the pressure of an ideal gas because of .....

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Match the Van der Waals constant $a$ (in $L^2 \cdot bar \cdot mol^{-2}$) for the following gases:

Gas $a$ value

$1. C_6H_{6(g)}$ $a. 0.217$

$2. C_6H_5CH_{3(g)}$ $b. 5.464$

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$4. H_2O_{(g)}$ $d. 24.060$

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