A 1.93-mol sample of xenon gas is maintained in a 0.805-L container at 306 K. Calculate the pressure of the gas using both the ideal gas law and the van der Waals equation (van der Waals constants for Xe are a = 4.19 L2atm/mol2 and b = 5.11×10-2 L/mol).

Answer : The pressure of the gas using both the ideal gas law and the van der Waals equation is, 60.2 atm and 44.6 atm respectively.

Explanation :

First we have to calculate the pressure of gas by using ideal gas equation.

where,

P = Pressure of gas = ?

V = Volume of gas = 0.805 L

n = number of moles  = 1.93 mole

R = Gas constant =

T = Temperature of gas = 306 K

Now put all the given values in above equation, we get:

Now we have to calculate the pressure of gas by using van der Waals equation.

P = Pressure of gas = ?

V = Volume of gas = 0.805 L

n = number of moles  = 1.93 mole

R = Gas constant =

T = Temperature of gas = 306 K

a = pressure constant =

b = volume constant =

Now put all the given values in above equation, we get:

Therefore, the pressure of the gas using both the ideal gas law and the van der Waals equation is, 60.2 atm and 44.6 atm respectively.