The pressure of a van der Waals gas is less t | vedclass

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(C) The ideal gas law assumes that there are no intermolecular forces of attraction or repulsion between gas molecules.However,real gases (van der Waa

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Intermolecular attraction

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(C) The ideal gas law assumes that there are no intermolecular forces of attraction or repulsion between gas molecules.However,real gases (van der Waals gases) exhibit intermolecular forces of attraction,known as van der Waals forces.These attractive forces pull the molecules inward,away from the walls of the container.Consequently,the molecules strike the container walls with less force than they would in the absence of these attractions.Therefore,the observed pressure of a real gas is lower than the pressure predicted for 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 van der Waals gas is less than the pressure of an ideal gas because of

Similar Questions

$A$ $Van \ der \ Waals$ real gas acts as an ideal gas under which of the following conditions?

In the given $pV \to V$ graph for gases at constant temperature,what kind of deviation will be observed for $H_2, He, CO, CH_4$?

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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

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

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

$3. Ne_{(g)}$ $c. 18.000$

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

The compressibility factor $(Z)$ of a gas is greater than unity at $1 \, atm$ and $273 \, K$. Therefore:

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