Why do real gases show deviation from ideal behaviour? Write van der Waals equation for ñ moles of a gas .
Answers
Explanation:
The causes of deviations from ideal behaviour may be due to the following two assumptions of kinetic theory of gases. The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas. The forces of attraction between gas molecules are negligible....
The van der Waals, equation for n moles of real gas is: `(P+(n^(2)a)/(V^(2)))(V - nb) = nRT` where P is the pressure, V is the volume , T is the absolute temperature, R is the molar gas constant and a, b are van der Waal's constant....
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Answer:
The causes of deviations from ideal behaviour may be due to the following two assumptions of kinetic theory of gases.
The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas.
The forces of attraction between gas molecules are negligible.