Nitrogen, when combined with oxygen, can form various oxides. 3.5 g of nitrogen gas is burned in oxygen to form 11.5 g of an oxide of nitrogen.
a) Determine the mass of oxygen burned. (Hint: The oxide contains ONLY nitrogen and
oxygen!)
b)Using the data from the experiment, find the percent of nitrogen by mass in the oxide.
c) Using the data from the experiment, find the percent of oxygen by mass in the oxide.
d) Use the data from this experiment to find the empirical formula of the oxide of nitrogen.
e) If you were given a 100. mg sample of the oxide, how many milligrams of nitrogen would
be in your sample?

c is the answer because when something is left after something evaporates that shows the chemical change.

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole