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QUESTION

# 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: