At 0 degrees celcius, a 1.0 L flask contains 5.0 x 10^-2 mol N2, 1.5 x 10^2 mg O2, 5.0 x 10^21 molecules NH3. Calculate the partial pressure of each gas and what is the total pressure in the flask.

Question

At 0 degrees celcius, a 1.0 L flask contains 5.0 x 10^-2 mol N2, 1.5 x 10^2 mg O2, 5.0 x 10^21 molecules NH3. Calculate the partial pressure of each gas and what is the total pressure in the flask.
How do I calculate this?

DrBob222 · Accepted Answer

Convert gases to mols.
You have mols N2.
mols O2 = grams/molar mass.
mols NH3 = # molecules/6.02E23

Plug each gas into PV = nRT (n = mols) and solve for the partial pressure of each gas. The total P is the sum of the partial pressures.