# Chem hw!

1. What pressure would be needed to compress 25.1 mL of hydrogen at 1.01 atm to 25% of its original volume?
2. If the pressure on a 1.04-L sample of gas is doubled at constant temperature, what will be the new volume of the gas?
3. A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expanded gas sample (at constant temperature)?
4. What pressure would have to be applied to a 27.2-mL sample of gas at 25 degrees celsius and 1.00 atm to compress its volume to 1.00 mL without a change in temperature?
5. How would you describe absolute zero?
6. A favorite demonstration in introductory chemistry is to illustrate how the volume of a gas is affected by temperature by blowing up a balloon at room temperature and then placing the balloon into a container of dry ice or liquid nitrogen (both of which are very cold). Suppose a balloon containing 1.15 L of air at 25.2 degrees Celsius is placed into a flask containing liquid nitrogen at -78.5 degrees celsius. What will the volume of the sample become (at constant pressure)?
7.Suppose a 1.25 L of argon is cooled from 291 K to 78 K. What will be the new volume of the argon sample?
8. Suppose a gas sample is cooled from 600 K to 300 K. Ho will the new volume of the gas be related to its original volume?
9. Th label of an aerosol spray can contains a warning that the can should not be heated to over 130 degrees F because of the danger of explosion due to the pressure increase as it is heated. Calculate the potential volume of the gas contained in 500-mL aerosol can when it is heated from 25 degrees C to 54 degrees C (approx. 130 degrees F) assuming a constant pressure.
10. A sample of gas has a volume of 127 mL in a boiling water bath at 100 degrees celsius. Calculate the volume of the sample of gas 10 degrees celsius intervals after the heat source is turned off and the gas sample begins to cool down to eh temperature of the laboratory, 20 degrees celsius.
11. At conditions of constant temperature and pressure, the volume of a sample of ideal gas is _____ proportional to the number of moles of gas present.
12. A mathematical expression that summarizes Avogadro's law is ________.
13. If 0.105 mol of helium gas occupies a volume of 2.35 L at a certain temperature and pressure, what volume would 0.337 mol of helium occupy under the same conditions?
14. If 1.00 mol of helium occupies a volume of 22.4 L at 273 K at 1.00 atm, what volume will 1.00 g of helium will occupy under the same conditions?
15. If 3.25 mol of argon gas occupies a volume if 100. L at a particular and temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions?
16. If 2.71 g of argon gas occupies a volume of 4.21 L, what volume will 1.29 mol of argon occupy under the same conditions?
17. If gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in an evacuated 1.04-L container at 25 degrees celsius, what will be the partial pressure of each gas and the total pressure in the container?
18. A tank contains a mixture of 3.0 mol of N2, 2.0 mol of O2, and 1.0 mol of CO2 at 25 degrees celsius and a total pressure of 10.0 atm. Calculate the partial pressure (in torr) of each gas in the mixture.
19. How many moles of helium gas would be required 2.14-L container to a pressure of 759 mm Hg at 25 degrees celsius? How many moles of neon gas would be required to fill a similar tank to the same pressure at 25 degrees celsius?
20. Calculate what mass of argon gas is required to fill a 20.4-L container to a pressure of 1.09 atm at 25 degrees celsius.
21. What is the pressure in a 245-L tank that contains 5.21 kg of helium at 27 degrees celsius?
22. What mass of helium gas is needed to pressurize a 100.0-L tank to a 255 atm at 25 degrees celsius? What mass of oxygen gas would be needed to pressurize a similar tank to the same specifications?
23. At what temperature will a 1.0 g sample of neon gas exert a pressure of 500. torr in a 5.0 L container?

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1. Show us the problem(s) you have tried to solve, one at a time, and someone will critique your thoughts.

This is not a place to drop off homework and pick up the answers before school.

These are mostly all exercises in using the ideal gas law, PV = nRT

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2. des

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3. If 0.105 mol of helium gas occupies a volume of 2.35 L at a certain temperature and pressure, what volume would 0.337 mol of helium occupy under the same conditions?

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4. Which of the following is NOT part of the kinetic theory of gases?
There is very little empty space in a gas.

The force of gas particles against the walls of a container is called
Pressure

A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mm Hg?

1140 mm Hg

The boiling point of water at sea level is 100°C. At higher altitudes, the boiling point of water will be
lower, because the atmospheric pressure is lower.

Vapor pressure can be described as

the pressure exerted by a gas above the surface of its liquid.

An autoclave is used to sterilize surgical equipment because
it allows water to boil at temperatures above 100°C.

Which of the following correctly describes the process of inspiration (air entering the lungs)?
The lungs expand, causing their internal pressure to decrease.

The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mm Hg. What is the final volume of the gas, assuming constant temperature? 4.6mL

Complete the following statement: In Charles' law, the volume of a gas ________ when the ________ decreases. Answer: decreases; temperature

The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure in the container is kept constant?
1170 mL

In Gay-Lussac's law, the pressure of a gas increases due to an increase in temperature because
the molecules strike the walls of the container more often.

At 570. mm Hg and 25°C, a gas sample has a volume of 2270 mL. What is the final pressure (in mm Hg) at a volume of 1250 mL and a temperature of 175°C? answer 1560 mm Hg

According to Avogrado's law, the volume of a gas is directly related to the number of moles at constant temperature and pressure.

At STP, temperature and pressure have the values of 273 K and 760 mm Hg.

A gas sample contains 4.0 g of CH4 and 2.0 g of He. What is the volume of the sample at STP?
17 L
A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15°C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27°C? 630 mL

How many moles of neon occupy a volume of 14.3 L at STP?

0.638 moles

1 mole of a gas occupies 22.4 L at

0°C and 760 mm Hg.

The total pressure in a mixture of gases is equal to the partial pressure(s) of

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mm Hg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr?
1100 torr

A tank contains helium gas at 490 mm Hg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?
2.1 atm

Which of the following correctly describes the partial pressures of gases in the body?
high O2, low CO2, oxygenated blood

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules
move rapidly in random directions.

As you rise higher in Earth's atmosphere, the atmospheric pressure
Decreases
At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 L to 3.00 L. What was the new pressure exerted by the helium on its container? 1270 torr

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25°C to 35°C. What was its new volume? 5.17 L

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0°C. During the summer, the temperature in the storage area reached 40.0°C. What was the pressure in the gas tank then? 5.63 atm
At STP, how many moles of helium would occupy 1.00 L? 0.0446 moles

If atmospheric pressure on a certain day is 749 mm Hg, what is the partial pressure of nitrogen, given that nitrogen is about 78% of the atmosphere? 584 mm Hg

A sample of argon at 300.°C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00°C. What is the new pressure? 23.8 atm

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