Gases which do not obey perfect gas love over a wide range of pressure and temperature are called real on an ideal gases. This deviations are due to interaction of molecules with each other and volume occupied by gas molecules. The repulsive forces between molecules assist expansion and attractive force assist compression.Deviation from ideal behaviour
the curve of the real gas has a tendency to conferred with that of an ideal gas at low pressure when the volume is large. At higher pressure however definitions are observed.
The behavior of real gases usually agrees with the predictions of the ideal gas equation to within 5% at normal temperatures and pressures. At low temperatures or high pressures, real gases deviate significantly from ideal gas behavior. ... It also assumes that the force of attraction between gas molecules is zero.
(c) Glass Possess fluidity is wrong.( According To Me)
(c) is the correct answer ok dear
1. one of the posulates of kinetic molecular theory of gasses is there are no attractive or repulsive forces among gas molecules.
this statement is not true, under high pressure and low temprature because, under these conditions the volume of gas is very very small and the distance between the molecules are also very small, as a result intermolecular forces develope which cannot be neglected. because of these intermolecular forces, the observed pressure is always smaller than that of ideal gas
2. One of the posulates of kinetic molecular theory of gasses is, the actual volume occupied by gas molecules is negligible when compared to the total volume of the gas. This statement is not true at higher pressure and lower temprature because at these conditions, the volume of gas is extremely small.
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
prefer to it child
Its shows that they have low temperature and pressure
Real gases deviate from ideal behaviour because their particles (atoms for inert gases or molecules) occupy some finite space and do exert interactive forces among them.
Completely ideal behaviour is hypothetical because of the reasons above.
At low pressure and high temperature, real gases behave approximately as ideal gases.
In ideal behaviour, gas particles don't occupy space and do not have any interaction, as assumed in the kinetic theory of gases.
But in reality this is not the case: we get errors by applying the ideal gas law. That's why van der Waals corrected it by introducing suitable constants.
HOPE YOU UNDERSTAND
Real gases do not obey ideal gas equation under all conditions. They nearly obey ideal gas equation at higher temperatures and very low pressures.
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.Please rate me 5 starsBM'S W