Question

A 1.4-L container of liquid nitrogen is kept in a closet measuring 1.1 m by 1.0...

A 1.4-L container of liquid nitrogen is kept in a closet measuring 1.1 m by 1.0 m by 1.9 m .

Assuming that the container is completely full, that the temperature is 27.6 ∘C, and that the atmospheric pressure is 1.0 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.)

Homework Answers

Answer #1

Ans- 1) the closet isn't sealed so that Pressure air initial = Pressure N2 vaporized = Pressure mixture final
2) the volumes are additive.. ie volume air + volume N2 vaporized = volume final
3) the composition of the final gas is uniform

volume air initially = (1.1m x 1.0m x 1.9m) x (1000L / m³) = 2090 L
volume N2 vaporized = nRT/P = (1.4L x 1000mL/L x 0.807g/mL x 1mole / 28.0g) x (0.082106 Latm/moleK) x (295.25K) / (1.1 atm) = 889.23 L

total volume = volume air + volume N2 vaporized = 2090L + 889.23 L = 2979.23 L

and that means only 2090L / 2979.23L = 70.15% of the air remains in the room and 29.85% of the air was displaced.
Assuming the mixture isn't uniform and that as a result, 1 L of N2 displaces 1 L of air, then 889.23 L of air was displaced. 889.23L / 2090L = 42.5% was displaced.
Of course N2 will diffuse about 7% faster than O2 due to it's molecular weight,
and the position of the container relative to any openings in the closet will play a factor in which gas escapes and of course air is indeed 79% N2. So you really can't distinguish between displacement of air molecules vs displacement of vaporized N2 molecules.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 1.5-L container of liquid nitrogen is kept in a closet measuring 1.0 m by 1.1...
A 1.5-L container of liquid nitrogen is kept in a closet measuring 1.0 m by 1.1 m by 1.9 m .Assuming that the container is completely full, that the temperature is 28.2 ∘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.)
A closed container with volume of 6.50 L holds 10.8 g of liquid helium at 3.00...
A closed container with volume of 6.50 L holds 10.8 g of liquid helium at 3.00 K and enough air to fill the rest of its volume at a pressure of 1.00 atm. The helium then evaporates and the container warms to room temperature (293 K). What is the final pressure inside the container? atm
1a. A sample of nitrogen gas in a 5.7-L container at a temperature of 19°C exerts...
1a. A sample of nitrogen gas in a 5.7-L container at a temperature of 19°C exerts a pressure of 3.1 atm. Calculate the number of moles of gas in the sample 1b. Given that 8.99 moles of carbon monoxide gas are present in a container of volume 30.90 L, what is the pressure of the gas (in atm) if the temperature is 95°C? 1c. Determine the molar mass of a gas with a density of 1.5877 g/L at 80.00°C and...
Liquid ethyl ether is introduced drop by drop into a 3.0 L closed container at 18...
Liquid ethyl ether is introduced drop by drop into a 3.0 L closed container at 18 degrees Celsius. After 122 drops of ethyl ether are added. No more evaporates and one drop is present in the container. What is the pressure in the container. The volume of one drop is 0.05 ml and the density of ethyl ether is 0.713 g/mL. The molar mass of ethyl ether is 74.12 g/ml. R=0.0821 The answer is 0.46 atm. Can you please show...
Trial Pressure( atm) Temperature(K) Reactant Mass Water displaced (L) Trial 1 NaHCO3 0.993 292.6K 1.0 g...
Trial Pressure( atm) Temperature(K) Reactant Mass Water displaced (L) Trial 1 NaHCO3 0.993 292.6K 1.0 g 0.163 L Trial 2 NaHCO3 0.993 292.8 K 1.1 g 0.122L Trial 3 Sodium Carbonate 0.993 292.7 K 0.9 g 0.125L Trial 4 Sodium Carbonate 0.993 279.5K 1.0 g 0.112L Beginning temp 293.15 Show your calculation for the molar volume of CO2 from Trial 1. 2, 3, 4 according to your experimental data. Show all work, values, and units in your calculations in order...
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What...
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What is the volume of the balloon when it ascends to an altitude where the temperature is -40. °C and 540. mmHg? 1 What volume does 12.5 g of Ar gas at a pressure of 1.05 atm and a temperature of 322 K occupy? Would the volume be different if the sample were 12.5 g of He gas under the same conditions? How many moles...
Procedure Reaction 1: Dissolving the Copper 1. Obtain a clean, dry, glass centrifuge tube. 2. Place...
Procedure Reaction 1: Dissolving the Copper 1. Obtain a clean, dry, glass centrifuge tube. 2. Place a piece of copper wire in a weighing paper, determine the mass of the wire and place it in the centrifuge tube. The copper wire should weigh less than 0.0200 grams. 3. In a fume hood, add seven drops of concentrated nitric acid to the reaction tube so that the copper metal dissolves completely. Describe your observations in the lab report. (Caution, Concentrated nitric...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT