Explore BrainMass

Explore BrainMass

    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.

    Not what you're looking for? Search our solutions OR ask your own Custom question.

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    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?

    © BrainMass Inc. brainmass.com November 24, 2022, 11:29 am ad1c9bdddf

    Solution Preview

    From the given data we can calculate the partial pressure of oxygen in the starting mixture:

    p(O2) = p - p(N2) = 2 atm - 1.5 atm = 0.5 atm

    where p = pressure of N2 and O2 mixture.
    According to Dalton's law of partial pressures we ...