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At 0.00 degrees C a 1.00 L flask contains 5.00 x 10^-2 mol N2, 1.50 x 10^2 mg O2, and NH3 at a concentration of 5.00 x 10^18 molecules/mL. What is the partial pressure of each gas, and what is the total pressure in the flask at atm?

  • chemistry -

    Convert mg and molecules to mols.
    mols N2 you have.
    mols O2 = grams/molar mass = ?
    mols NH3 = #molecules/6.02E23 = ?

    Use PV = nRT and solve for each pressure.
    Then total P = sum of partial pressures.

  • chemistry -

    Thank you very much!

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