van der Waal's equation for calculating the pressure of a non ideal gas is
`(P+(an^(2))/(V^(2)))(V-nb)=nRT`
van der Waal's suggested that the pressure exerted by an ideal gas , `P_("ideal")`, is related to the experiventally measured pressure, `P_("ideal")` by the equation
`P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2))))`
Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas .
Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows :
`underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT`
AT relatively high pressures, the van der Waals' equation of state reduces to

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT Using van der Waals' equation, find the constant 'a' (in atm L^(2)mol^(-2) ) when two moles of a gas confined in 4 L flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L mol^(-1) .(R = 0.082 atm.L/K mol)

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT The van der Waals' constant 'a' for CO_(2) gas is greater than that of H_(2) gas. Its mean that the

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT For non-zero value of force of attraction between gas moleculer at large volume, gas equation will be :

The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT

The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb) = nRT

Write the van der Waals equation for 5 mole of ideal gas.

Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

Units of a and b in van der Waal's equation (P+(an^(2))/(V^(2)))(V-nb)=nRT are

van der Waal's equation reduces itself to the ideal gas equation at