Difficult
Give two unfair assumptions of the Kinetic Molecular Theory of gases. Justify them.
(N/A) The two main unfair assumptions of the Kinetic Molecular Theory of gases are:
$1$. The volume occupied by gas molecules is negligible compared to the total volume of the gas.
Justification: At high pressures,the gas molecules are pushed close together,and their actual volume becomes significant relative to the total volume of the container.
$2$. There are no forces of attraction or repulsion between gas molecules.
Justification: At low temperatures and high pressures,gas molecules move slowly and come closer to each other,leading to significant intermolecular forces of attraction,which causes the gas to deviate from ideal behavior and eventually liquefy.
$1$. The volume occupied by gas molecules is negligible compared to the total volume of the gas.
Justification: At high pressures,the gas molecules are pushed close together,and their actual volume becomes significant relative to the total volume of the container.
$2$. There are no forces of attraction or repulsion between gas molecules.
Justification: At low temperatures and high pressures,gas molecules move slowly and come closer to each other,leading to significant intermolecular forces of attraction,which causes the gas to deviate from ideal behavior and eventually liquefy.
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