Calculate the pressure exerted by 0.5000 mol of n2 in a 1.-l container at 25.08c a. using the ideal gas law. b. using the van der waals equation. c. compare the results.

Explanation:

a).  According to ideal gas equation, product of pressure and volume is equal to the product of number of moles, gas constant and temperature.

Mathematically,         PV = nRT

Since, it is given that number of moles is 0.5 mol, volume is 1.0 L and temperature is . Or in kelvin temperature will be (25.08 + 273) K = 298.08 K.

Therefore, to calculate the pressure put the given vaues in the ideal gas equation as follows.

                       PV = nRT

                  = 0.5 mol \times 0.0821 L atm/mol K \times 298.08 K[/tex]

                      P = 12.236 atm

                         = 12.24 atm (approx)

b).   Vander waal equation is as follows.

                    = RT

For nitrogen gas, value of a is 1.370 and b is 0.0387. Therefore, putting the given values into Vander waal's equation as follows.

                    = RT

                    P =

                    P =

                     P = 12.14 atm

c).   Pressure calculated using ideal gas equation is 12.24 atm. Whereas pressure calculated using Vander waal's equation is 12.14 atm.

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