Respuesta :
Answer:
E. All of the above statements are correct
Explanation:
The gas equation given below and which we are familiar with relates to ideal gases and not to real gases .
P V = R T
In this equation , it has been assumed that gas molecules have no mutual attraction . They do not occupy any space ie they are very small in volume . But in reality , gas molecules do have mutual attraction and also they occupy some space. . Considering these facts , a new formula was given to replace the gas equation which is written below .
(P - a / V² ) ( V - b ) = R T , a and b are constant and depend upon nature of gas involved .
This is called van der Waals equation . This is for one mole .
Here we see P of previous gas equation is replaced by P - a / V² .
That means pressure of real gas is less than the ideal gas . It is due to mutual attraction between any two gas molecules. V of previous gas equation is replaced by V - b . That means volume of empty space has been reduced . It is due to the fact that real gas molecules occupy some space . Here b is dependent on the nature of the gas.
So all the statements are correct .
The van der Waals equation for real gases recognizes that gas particles have non-zero volumes and interact with one another.
The ideal gas equation is used to describe the relation among the volume, pressure and temperature of an ideal gas. Recall that the ideal gas equation holds that there is no intermolecular interaction between gas molecules and that gas molecules occupy zero volume relative to the volume of the container.
The van der Waals equation for real gases recognizes that gas particles have non-zero volumes and interact with one another.
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