Review example 5.10 and exercise 5.10. Suppose 1.58 moles of N2 and 0.420 moles of O2 occupy 22.41 L at a total pressure of 2.00 atm.

Question

Use XA = to determine the (decimal) mole fractions of both components.
Then, use XA = to determine the partial pressures (PA) of both components.
Show all applicable units.

How would you get the total moles? I know you have to divide moles of O2 by total moles I got 0.013 then I divided 1.58 moles if N2 by 28 and I got 0.06. Is this right? Then the formula would be XO2 =pO2/ptotal right

Answer 1

Total mols = mols O2 + mols N2 = 1.58 + 0.420 = ?
You divided mols/molar mass to find X and that isn't right.
XO2 = nO2/total mols.
XN2 = nN2/total mols
Then you can find partial pressure of each this way.
pO2 = XO2*Ptotal
pN2 = XN2*Ptotal