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.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.