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PART A: Three gases (8.00 g of methane, C H 4 , 18.0 g of ethane,...

PART A:

Three gases (8.00 g of methane, C H 4 , 18.0 g of ethane, C 2 H 6 , and an unknown amount of propane, C 3 H 8 ) were added to the same 10.0- L container. At 23.0 ∘ C , the total pressure in the container is 3.80 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 30.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 665 mmHg ?

Express you answer numerically in millimeters of mercury.

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Answer #1

PART A The total number of moles of gases present in the 10.0-L container is calculated by the following formula PV nRT PV RT

18.0 Number of moles of ethane 30.0 g/mol 0.6mol shown below The number of moles of propane is calculated as Number of moles

The partial pressure of methane, ethane, propane is 1.121 atm, 1.218 atm, 1.462 atm respectively PART B contains 30.8 % nitro

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