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?

Answer 1

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.

Answer 2

Thank you very much!