Chemistry

posted by .

A gas mixture containing N2 and O2 was kept inside a 2 L container at a temperature of 23 C and a total pressure of 1 atm. The partial pressure of oxygen was .722 atm. How many grams of nitrogen were present in the gas mixture?

  • Chemistry -

    Ptotal = pN2 + pO2
    You know pO2, solve for pN2.

    Substitute pN2 into PV = nRT and solve for n. Then
    n = mols = grams/molar mass.
    You know mols and molar mass; solve for grams N2.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemsitry II

    The partial pressure of CH4(g) is 0.185 atm and that of O2(g) is 0.300 atm in a mixture of the two gases. a) What is the mole fraction of each gas in the mixture?
  2. Chemsitry II

    mole fraction is equal to partial pressure divided by the total pressure Total pressure= sum of partial pressure use PV=nRT where n= number of moles equation become PV/RT=n make sure to convert the temperature to Kelvin and to use …
  3. Chemistry

    Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.6 L of water upon warming from 25 C to 50 C. Assume that the water is initially saturated with nitrogen …
  4. Chemistry

    Sulfur dioxide is used to make sulfuric acid. one method of producing it is by roasting mineral sulfides, for example, FeS2(s) + O2 (g) ---> SO2(g) + Fe2O3(s) (unbalanced). A production error leads to the sulfide being placed in …
  5. chemistry

    A gaseous mixture in a 25.00 L container is made of 16.0 g N2 and 14.0 g Ar and has a total pressure of 1.00 atm. 1.Calculate the partial pressure of the N2 in the mixture. the ans is 0.620 atm 2.Calculate the temperature of the gas …
  6. chemisrty

    Q6) A 10 L container contains a mixture of 0.8 g of He and 8 g of Ar at 0 oC. a) (1 pt) Calculate the total pressure of the gas mixture. b) (1 pt) Calculate the partial pressure of each gas in the gas mixture. c) (1 pt) If the initial …
  7. Chemistry

    a gas misture containing N2 and O2 was kept inside a 2.00 L container at a temp of 23.0 degrees C and a total pressure of 1.00atm. The partial pressure of O2 was 0.722atm. How many grams of Nitrogen were present in the mixture?
  8. Chemistry

    A mixture of 1.39 g H2 and 1.60 g He is placed in a 1.00-L container at 27°C. Calculate the partial pressure of each gas and the total pressure. PH2 = ?
  9. chem 102

    Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.1L of water upon warming from 25 ∘C to 50 ∘C. Assume that the water is initially saturated …
  10. chemistry 116

    You have a rigid sealed container held at a constant temperature. You add 3.3 atm of oxygen gas, 1.7 atm of nitrogen and 4.2 atm of methane to it. What is the partial pressure of the oxygen gas in the container

More Similar Questions