Determining the initial mole and mass fractions of oxygen and nitrogen in a mixture using Dalton's law of partial pressure. Solution in MS Word.
A reaction vessel contained 5 liters of a mixture of N2 and O2 gases at 25oC and 2 atm pressure. The oxygen in the mixture was completely removed by causing it to oxidize with an excess of electrically heated zinc wire contained in the vessel to non-volatile solid ZnO. The pressure of N2 that remained (measured again at 25oC) was 1.5 atm. What were the mole and mass percent of O2 in the starting mixture?© SolutionLibrary Inc. solutionlibary.com 9836dcf9d7 https://solutionlibrary.com/chemistry/physical-chemistry/determining-the-initial-mole-and-mass-fractions-of-oxygen-and-nitrogen-in-a-mixture-using-daltons-law-of-partial-pressure-solution-in-ms-word-1ad
...2) = x(O2)*p
where p(O2) is partial pressure of O2 in the mixture, x(O2) is mole fraction of oxygen in the mixture and p is total pressure of mixture. Hence:
x(O2) = p(O2)/p = 0.25 or 25%.
To find mass percent we have to convert moles ...