AP Matter Class Packet Unit 5


Gases Review

KMT is the study of how ideal or ______gases behave. Real gases behave most like ideal gases under ______pressure and ______temperature.

1.  Based on the demonstration performed by your teacher, describe how gas molecules behave:

Motion: ______

Collisions: ______

Volume: ______

Attractions: ______

2.  How can you get a real gas to behave the LEAST like an ideal gas?

3.  Of the following: H2, He, CO2, which would behave least like and ideal gas and why?

4.  Which of the gases in question 3 behaves the most like ideal gases/ Why?

5.  Compared to other gases, why doesn’t water vapor behave ideally?

6.  Why do gases behave the least like ideal gases at low temperatures and high pressures?

Combined Gas Law

  1. If the temperature of a 50mL sample of a gas is changed from 200K to 400K under constant pressure, what is the new volume of the gas?
  1. The volume of a gas is 204mL when the pressure is 925kPa. At constant temperature, what is the final pressure if the volume increases to 306ml?
  1. A 1.53L sample of sulfur (IV) oxide at a pressure of 5.60kPa. If the pressure is changed to 15.0kPa at constant temperature, what will be the new volume of the gas? Assume temperature is constant.
  1. The Hindenburg exploded in 1937. It held 2.0x105 m3 of hydrogen gas at 23C at standard pressure. How much gas would that be at standard pressure on a warm day of 45C?
  1. An aerosol spray can with a volume of 456mL contains 3.18g of propane gas as a propellant. If the can is at 23C, and 0.50atm, what volume would the propane occupy at STP?
  1. Suppose the P and T was tripled on a 6.0L sample of a gas. What is the new volume?

7.  A gas has a volume of 50. mL at a temperature of 10.0 K and a pressure of 760. kPa. What will be the new volume when the temperature is changed to 20.0 K and the pressure is changed to 380. kPa?

8.  The volume of a sample of a gas at 273 K is 100.0 L. If the volume is decreased to 50.0 L at constant pressure, what will be the new temperature of the gas?

9.  A gas has a volume of 2.00 L at 323 K and 3.00 atm. What will be the new volume if the temperature is changed to 273 K and the pressure is changed to 1 atm?

10.  What will be the new volume of 100. mL of gas if the Kelvin temperature and the pressure are both halved?

11.  A gas occupies a volume of 500. mL at a pressure of 380. kPa and a temperature of 298 K. At what temperature will the gas occupy a volume of 250. mL and have a pressure of 760. kPa?

12.  A gas at STP has a volume of 1.00 L. If the pressure is doubled and the temperature remains constant, what is the new volume of the gas?

13.  A cylinder of a car’s engine has a volume of 0.725 L when the piston is at the bottom of the cylinder. When the piston is at the top of the cylinder it has a volume of 0.050L. If the cylinder is filled with air at a pressure of 1 atm when the piston is at the bottom, what is the pressure when the piston is at the top if the temperature remains constant?

  1. A sample of gas is held at constant pressure. Increasing the kelvin temperature of this gas sample causes the average kinetic energy of its molecules to
  2. decrease and the volume of the gas sample to decrease
  3. decrease and the volume of the gas sample to increase
  4. increase and the volume of the gas sample to decrease
  5. increase and the volume of the gas sample to increase
  1. A sample of helium gas has a volume of 900. milliliters and a pressure of 2.50 atm at 298 K. What is the new pressure when the temperature is changed to 336 K and the volume is decreased to 450. milliliters?
  2. 0.177 atm b. 4.43 atm c. 5.64 atm d. 14.1 atm
  1. A gas occupies a volume of 444 mL at 273 K and 79.0 kPa. What is the final kelvin temperature when the volume of the gas is changed to 1880 mL and the pressure is changed to 38.7 kPa?
  2. 31.5 K b. 292 K c. 566K d. 2360K

Graham’s Law of Diffusion

1.  At STP, which gas diffuses at the faster rate?

A) H2 B) N2 C) CO2 D) NH3

2.  Under the same conditions of temperature and pressure, which gas will diffuse at the slowest rate?

A)  He B) Ne C) Ar D) Rn

3. Which gas would diffuse most rapidly under the same conditions of temperature and pressure?

A)  gas A, molecular mass = 4 C) gas B, molecular mass = 16

B)  gas C, molecular mass = 36 D) gas D, molecular mass = 49

4.  Arrange the following gas in order of increasing average molecular speed at 25C: He, O2, CO2, H2O.

Avogadro’s Law

1.  The table below shows mass and volume data for four samples of substances at 298 K and 1 atm.

Which two samples could consist of the same substance?

A)  A and B C) A and C

B)  B and C D) C and D

2.  A sample of oxygen gas is sealed in container X. A sample of hydrogen gas is sealed in container Z. Both samples have the same volume, temperature, and pressure. Which statement is true?

A)  Container X contains more gas molecules than container Z.

B)  Container X contains fewer gas molecules than container Z.

C)  Containers X and Z both contain the same number of gas molecules.

D)  Containers X and Z both contain the same mass of gas.

3.  At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO2(g) have

A)  equal masses and the same number of molecules

B)  different masses and a different number of molecules

C)  equal volumes and the same number of molecules

D)  different volumes and a different number of molecules

4.  Each stoppered flask to the right contains 2 liters of a gas at STP. Each gas sample has the same

A)  Density B) mass C) number of molecules D) number of atoms

Dalton’s Law of Partial Pressures

1. Gases X, Y, and Z, in a closed system at constant temperature, have a total pressure of 80 kPa. The partial pressure of each gas is shown below.

The partial pressure of gas X, in kPa, is equal to

A) B)

C) D)

2. What is the pressure of a mixture of CO2, SO2, and H2O gases, if each gas has a partial pressure of 25 kPa?

A)  25 kPa B) 50 kPa C) 75 kPa D) 101 kPa

3. A flask contains a mixture of N2(g) and O2(g) at STP. If the partial pressure exerted by the N2(g) is 40.0 kPa, the partial pressure of the O2(g) is

A)  21.3 kPa B) 37.3 kPa C) 61.3 kPa D) 720 kPa

4. Gas samples A, B, and C are contained in a system at STP. The partial pressure of sample A is 38.0 kPa and the partial pressure of sample B is 19.0 kPa. What is the partial pressure of sample C?

A)  19.0 kPa B) 38.0 kPa C) 44.3 kPa D) 63.3 kPa

5. The partial pressures of gases A, B, and C in a mixture are 0.750 atmosphere, 0.250 atmosphere, and 1.25 atmospheres, respectively. What is the total pressure of the gas mixture in kPa?

A)  2.25 kPa B) 202 kPa C) 228 kPa D) 301 kPa

6.  A mixture of oxygen, nitrogen, and hydrogen gases exerts a total pressure of 74 kPa at 0ºC. The partial pressure of the oxygen is 20 kPa and the partial pressure of the nitrogen is 40 kPa. What is the partial pressure of the hydrogen gas in this mixture?

A)  14 kPa B) 20 kPa C) 40 kPa D) 74 kPa

7.  A mixture of gases contains 0.75mol nitrogen, 0.30mol oxygen, and 0.15 mol of carbon dioxide. If the total pressure is 2.3atm, what are the partial pressures?

Ideal Gas Law

1.  A 7.8g piece of solid carbon dioxide is placed in a 4.0L container at 27 degrees Celsius. What is the pressure in atmospheres in the container after all the carbon dioxide vaporizes?

2.  Automobile air bags inflate when sodium azide (NaN3) decomposes into its elements. If 97.5g of sodium azide are added to an air bag that will inflate to a volume of 0.30L and heat up to 100.C, then what is the pressure exerted on the bag by the nitrogen gas produced in the reaction?

3.  Using the Haber process to produce ammonia gas, you can obtain the greatest yield of ammonia at high temperatures and pressures, but it is dangerous, so lower T and P is used. Typically, the Haber process is performed at 500C and 250 atmospheres. Assuming the reaction goes to completion, what volume would ammonia occupy if 21.0g of nitrogen is reacted with excess hydrogen?

4.  The Hindenburg exploded in 1937. It held 2.0x105 m3 of hydrogen gas at 23C and standard pressure what mass of hydrogen was present?

5.  A scuba diver's tank contains 0.29kg of oxygen compressed into a volume of 2.3L. What is the pressure in the tank a 9C?

Ideal Gas Law with Density

1.  What is the density of nitrogen gas at 1.50atm and 298K?

2.  A 44.8L balloon is filled with Helium with a pressure of 1atm at 25C. What is the density of the gas?

3.  An AP student decided to bribe me with cookies for a better grade. He allowed the yeast to ferment so the dough will rise. If 200.0g of glucose (sugar) is used at standard pressure and 30C what is the volume of carbon dioxide gas produced? What is the density?

4.  Which gas is most dense at 1.00atm and 298K? CO2, N2O, or Cl2?

5.  What is the density of NO2 gas at 0.970 atm and 35C?

AP Gas Problems

1. A mixture of H2(g), O2(g), and 2 millilitres of H2O(l) is present in a 0.500 litre rigid container at 25°C. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1,146 millimetres mercury. (The equilibrium vapor pressure of pure water at 25°C is 24 millimetres mercury.)

The mixture is sparked, and H2 and O2 react until one reactant is completely consumed.

(a) Identify the reactant remaining and calculate the number of moles of the reactant remaining.

(b) Calculate the total pressure in the container at the conclusion of the reaction if the final temperature is 90°C. (The equilibrium vapor pressure of water at 90°C is 526 millimetres mercury.)

(c) Calculate the number of moles of water present as vapor in the container at 90°C.

2. Observations about real gases can be explained at the molecular level according to the kinetic molecular theory of gases and ideas about intermolecular forces. Explain how each of the following observations can be interpreted according to these concepts, including how the observation supports the correctness of these theories.

(a) When a gas-filled balloon is cooled, it shrinks in volume; this occurs no matter what gas is originally placed in the balloon.

(b) When the balloon described in (a) is cooled further, the volume does not become zero; rather, the gas becomes a liquid or solid.

(c) When NH3 gas is introduced at one end of a long tube while HCl gas is introduced simultaneously at the other end, a ring of white ammonium chloride is observed to form in the tube after a few minutes. This ring is closer to the HCl end of the tube than the NH3 end.

(d) A flag waves in the wind.

3. A student collected a sample of hydrogen gas by the displacement of water as shown by the diagram above. The relevant data are given in the following table.

GAS SAMPLE DATA
Volume of sample / 90.0 mL
Temperature / 25°C
Atmospheric Pressure / 745 mm Hg
Equilibrium Vapor Pressure of H2O (25°C) / 23.8 mm Hg

(a) Calculate the number of moles of hydrogen gas collected.

(b) Calculate the number of molecules of water vapor in the sample of gas.

(c) Calculate the ratio of the average speed of the hydrogen molecules to the average speed of the water vapor molecules in the sample.

(d) Which of the two gases, H2 or H2O, deviates more from ideal behavior? Explain your answer.

4.

Represented above are five identical balloons, each filled to the same volume at 25°C and 1.0 atmosphere pressure with the pure gases indicated.

(a) Which balloon contains the greatest mass of gas? Explain.

(b) Compare the average kinetic energies of the gas molecules in the balloons. Explain.

(c) Which balloon contains the gas that would be expected to deviate most from the behavior of an ideal gas? Explain.

(d) Twelve hours after being filled, all the balloons have decreased in size. Predict which balloon will be the smallest. Explain your reasoning.



Solutions Review