A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total pressure of 2.95 atm. What is the?

Question

pressure of H2?

Isn't is something like total pressure (TP) - T1 - T2?

Please help me understand how to do this. I really want to learn this stuff!

Answer 1

Total moles = 0.220 + 0.350 + 0.640 = 1.21 mol

The pressure of H2 = 0.350 mol / 1.21 mol x 2.95 atm

= 0.85 atm

Answer 2

n = 0.220 + 0.350 + 0.640 = 1.21 mole

H2 = 0.350 mol

pressure of H2 = 2.95 atm x (0.350 mol/1.210 mol) = 0.853 atm

1 mol of any ideal gas will have the same pressure if the T and V are constant. The total pressure is 2.95 atm. Each gas contributes to the pressure based on its mole fraction.

The mole fraction of H2 = 0.350 / 1.210 = 0.2893

The mole fraction of CO = 0.220 / 1.210 = 0.1818

The mole fraction of He = 0.640 / 1.210 = 0.5289