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 4.40 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. A gaseous mixture of O2 and N2 contains 37.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 265 mmHg ? Express you answer numerically in millimeters of mercury.
a) First calculate total moles using total pressure,
Mole Fraction of Each Components:
Partial Pressure of each components:
Let total mass of mixture be 100g.
Mass of O2 = 62.2 g
Moles of O2 = 62.2 / 32 = 1.943
Mass of N2 = 37.8 g
Moles of N2 = 37.8 / 28 = 1.35
Mole Fraction of Components:
Partial Pressure of Components:
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