Can you explain the deviation of real gases using Van der Waals equation?

##Van## ##der## ##Waals## ##equation##:

Van der Waals equation is used with amendment of ideal gas

Equation:

Amendment for volume:

Volume of an ideal gas ##V##.When the *real * gas is kept in that ##V## volume ,volume occupied by real gas is ##x##. Then the volume of an ideal gas is ##(V-x)##

Amendment for pressure:

Pressure of an ideal gas is ##P##. Measured pressure of real gas is ##p##. Pressure reduced due to intermolecular attraction of real gas is ##y##. If we add measured pressure of real gas and pressure reduced due to intermolecular attraction of real gas is equal to the the pressure of ideal gas.

##P=p+y##

Therefore Van der Waals equation is:

##a## and ##V## are constants for real gases. This equation can be used in any temperature and pressure.

This equation is equal to ideal gas at high tempareture and low pressure. Because:

##p##+##a##(##n^2##/##v^2##) is almost equal to ##p## and ##V-nb## is almost equal to ##V##

becuase So for real gases,

##a## & ##V## are constant. Therefore, they deviate from ideal gas behavior.

Deviation is as follows: