1. Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown a
ID: 867568 • Letter: 1
Question
1. 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 4.50atm . 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.
2. A gaseous mixture of O2 and N2 contains 40.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 425mmHg ? Express you answer numerically in millimeters of mercury.
Explanation / Answer
1.
partial pressure= P of the gas/total P
mol CH4= 8g/16g/mol= 0.5 mol
mol C2H6= 18g/30g/mol= 0.6 mol
PCH4=0.5 mol x 0.082L.atm/mol.K x 296K/ 10L= 1.2136 atm
PC2H6= 0.6 mol x 0.082L.atm/mol.K x 296K/ 10L= 1.4563 atm
Ptotal=4.5 atm= 1.2136 atm + 1.4563 atm + PC3H8 ---> PC3H8= 1.8301atm
PPCH4= 1.2136/4.5=0.270
PPC2H6= 1.4563/4.5= 0.323
PPC3H8= 1.8301/4.5= 0.407
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According with Chegg rules, when there are more than 1 question on the post we have to answer just the first one, really sorry :(
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