Question

Part 1. The air in a bicycle tire is bubbled through water and collected at 25∘C.

If the total volume of gas collected is 5.60 L at a temperature of 25∘C and a pressure of 760 torr, how many moles of gas were in the bicycle tire?

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Part 2. A 295-mL flask contains pure helium at a pressure of 755 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 714 torr.

a. If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of helium?

b. If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of argon?

c. If the two flasks are connected through a stopcock and the stopcock is opened, what is the total pressure?

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Part 3. A 1.00 L flask is filled with 1.30 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.100 atm.

a. What is the partial pressure of argon in the flask?

b. What is the partial pressure of ethane in the flask?

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Part 4. An experiment shows that a 111 mL gas sample has a mass of 0.171 g at a pressure of 747 mmHg and a temperature of 34 ∘C.

What is the molar mass of the gas?

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Part 5. Use the molar volume of a gas at STP to calculate the density of carbon dioxide gas at STP. Express the density in grams per liter to three significant figures.

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Part 6. A 1.5-L container of liquid nitrogen is kept in a closet measuring 1.2 m by 1.0 m by 1.8 m.

Assuming that the container is completely full, that the temperature is 24.7 ∘C, and that the atmospheric pressure is 1.1 atm, calculate the percent (by volume) of air that would be displaced if all of the liquid nitrogen evaporated. (Liquid nitrogen has a density of 0.807 g/mL.)