Dalton's law states that the total pressure, Ptotal, of a mixture of gases in a container equals the sum of the pressures of each individual gas:

Ptotal = P1+ P2+ P3+

The partial pressure of the first component, P1, is equal to the mole fraction of this component, X1, times the total pressure of the mixture:

P1 = X1 Ptotal

The mole fraction, X, represents the concentration of the component in the gas mixture, so:

X1 = moles of component 1 / total moles in mixture

Part A: Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8 were added to the same 10.0-L container. At 23.0 C, the total pressure in the container is 5.50 atm. Calculate the partial pressure of each gas in the container.

Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane.

Part B: A gaseous mixture of O2 and N2 contains 31.8 %nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 805 mmHg ?

Express you answer numerically in millimeters of mercury.