Question #179197

Write the equation of the corresponding states and explain the meaning of the terms involved in it.

Expert's answer

Ideal gas equation of state is PV =RT for one mole of gas

Van der Waals equation of state proposed the following equation to explain the P-V-T behaviour of real gases

The pressure term in ideal gas equation replaced by P + (a/V^{2})

and Volume term is replaced by (V - b )

Where b is the volume per mole of the gas

(P + a/V^{2})(V-b) = RT

V is the molar volume of the gas

V_{C} = 3b,. T_{C } = 8a/27Rb.

P_{C} = (RT_{C}/2b)-(a/9b^{2})

on solving equations of T_{C} and V_{C} we get Van der Waals constants as

a= 27R^{2}T_{C}^{2}/64P_{C}

b= RT_{C}/8P_{C}

T_{C }and P_{C} are critical temperature and critical pressure

a and b are the van der Waals constant

P is the actual pressure of the gas

The principal states that all gases when compared at the same reduced temperature and the reduced pressure, have approximately the same compressibility factor and all deviate from the ideal behaviour to the same extent

Reduced pressure P_{r} = P/P_{C}

Reduced temperature T_{r} = T/T_{C }and

Reduced Volume V_{r} = V/V_{C}

Where V, T and P are the actual Volume, temperature and pressure

(P_{r }+ 3/V_{r}^{2})(3V_{r} - 1) = 8T_{r} ________(a)

above equation is known as Van der Waals equation of state in reduced formed

Learn more about our help with Assignments: Inorganic Chemistry

## Comments

## Leave a comment