chapter 13 gases day plans for the day...

Chemistry Name __________________________

Hour _______

Chemistry

Approximate Timeline

Students are expected to keep up with class work when absent.

CHAPTER 13 – GASES

Day Plans for the day Assignment(s) for the day

1 Begin Chapter 13

13.1 – Describing the Properties of Gases

Pressure, Temperature, & Volume

o Pressure & Volume: Boyle’s Law

Demo – syringe

Assignment 13.0

Assignment 13.1a

2 13.1 – Describing the Properties of Gases

o Volume & Temperature: Charles’ Law

Demo – crushing a soda can

Assignment 13.1b

3 13.1 – Describing the Properties of Gases

o Volume & Moles: Avogadro’s Law

Assignment 13.1c

Read section(s) 13.2

4 13.2 – Using Gas Laws to Solve

Problems

o The Ideal Gas Law

Assignment 13.2a


Problems

o Dalton’s Law of Partial Pressures

Assignment 13.2b

Read section(s) 13.3


Problems

o Gas Stoichiometry

Assignment 13.2c

7 13.3 – Using a Model to Describe Gases

o Laws & models: a Review

o The Kinetic Theory of Gases

o Implications of the Kinetic Theory

o Real Gases

Assignment 13.3

8 Work on Assignment 13.4 Assignment 13.4

9 Grade & discuss Assignment 13.4

Review for Chapter 13 Test

10 Chapter 13 Test Read section(s) 15.1

Chemistry Name __________________________

Hour _______

Study Guides

Chapter 13 Quizzes

Quiz 13.1ab Pressure & Boyle’s Law 1. Define the term “barometer”.

2. Who invented the mercury barometer?

3. Give three different units of pressure.

4. State Boyle’s Law.

5. Write Boyle’s Law as a mathematical equation.

6. If the pressure on a gas is increased, the volume of the gas ___.

7. If the pressure on a gas is doubled, the volume of the gas ___.

8. Be able to solve a Boyle’s Law problem.

Quiz 13.1cd Charles’s Law & Avogadro’s Law 9. State Charles’s Law.

10. Write Charles’s Law as a mathematical equation.

11. If the temperature of a gas is increased, the volume of the gas ___

12. If the temperature of a gas is doubled, the volume of the gas ___

13. Which temperature scale resulted from Charles’s experiments? ___

14. State Avogadro’s Law.

15. Write Avogadro’s Law as a mathematical equation.

16. If the number of moles of gas is increased, the volume of the gas ___

17. If the number of moles of gas is doubled, the volume of the gas ___

18. Be able to solve a Charles’s Law problem.

19. Be able to solve an Avogadro’s Law problem.

Quiz 13.2ab Ideal Gas Law, Combined Gas Law, & Dalton’s Law 20. Write the ideal gas law as a mathematical equation.

21. Define the term “ideal gas.”

22. State Dalton’s Law of Partial Pressures.

23. Write Dalton’s law as a mathematical equation.

24. Be able to solve an Ideal Gas Law problem.

25. Be able to solve an Dalton’s Law problem.

Quiz 13.2c Gas Stoichiometry 26. Define the term “molar (gas) volume.”

27. What does the acronym “STP” stand for?

28. What is the value of standard temperature?

29. What is the value of standard pressure?

30. Be able to solve all three types of gas stoichiometry problems.

Quiz 13.3 Using a Model to Describe Gases 31. The “kinetic molecular theory attempts to explain the behavior of gases in terms of ___

(a long phrase).

32. Think about the kinetic molecular theory and answer the following.

a. As the temperature increases the molecules move ___

b. As the temperature increases the pressure ___

c. As the temperature increases the volume ___

Chemistry Name __________________________

Hour _______

Study Guide

Chapter 13 Test

Chemistry

At the completion of chapter 13 you should…

1. Know the definitions of the following terms.

a. Boyle’s Law

b. Charles’s Law

c. Avogadro’s Law

d. Dalton’s Law

e. Molar Gas Volume

f. Absolute Zero

g. Torr

h. Ideal Gas

i. STP

j. Kinetic Molecular Theory

2. Be able to state Boyle’s Law in words and as a mathematical equation.

3. Be able to state Charles’s Law in words and as a mathematical equation.

4. Be able to state Avogadro’s Law in words and as a mathematical equation.

5. Be able to state Dalton’s Law in words and as a mathematical equation.

6. Know what is meant by “molar gas volume” and its value at STP.

7. Know the significance of absolute zero.

8. Know the two assumptions of an ideal gas.

9. Know what STP stands for and its values.

10. Be able to solve all types of gas law problems

a. Boyle’s Law

b. Charles’s Law

c. Avogadro’s Law

d. Dalton’s Law

e. Ideal Gas

f. Combined Gas Law

g. Gas stoichiometry

11. Know the conditions under which real gas behavior is different than that of an ideal gas.

Chemistry Name __________________________

Hour _______

Assignment 13.0 – Vocabulary

Define each of the following terms.

1. Boyle’s Law (words & equation)

2. Charles’s Law (words & equation)

3. Avogadro’s Law (words & equation)

4. Dalton’s Law (words & equation)

5. Molar Gas Volume

6. Absolute Zero

7. Torr

8. Ideal Gas

9. STP

10. Kinetic Molecular Theory

Chemistry Name __________________________

Hour _______

Assignment 13.1a – Boyle’s Law Solve each of the following problems. In order to receive full credit you must do three things: (1)

write the equation, (2) plug in the numbers with units, and (3) circle your answer expressed

with the correct number of significant digits and units.

1) At 25°C and 150 kPa a gas occupies 325 mL. What volume will the gas occupy at

standard pressure if the temperature remains constant?

2) A sample of chlorine gas occupies 100.0 mL at standard pressure. The pressure is

changed so that the gas now occupies 147.0 mL. What is the new pressure?

3) At a pressure of P1 a gas occupies 90.0 mL. At a pressure of 78.1 kPa the gas occupies

190.0 mL. If the temperature stays the same, what is the value of P1?

4) At standard pressure a sample of neon occupies 125 mL. What volume will it occupy at

125 kPa? Assume constant temperature.

5) At constant temperature and 1794 kPa a sample of helium occupies 2.98 mL. What

volume will it occupy at 49.71 kPa?

Chemistry Name __________________________

Hour _______

Assignment 13.1b – Charles’s Law Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) At 25°C a sample of oxygen occupies 123 L. What volume will it occupy at standard

temperature if the pressure is held constant?

2) A sample of oxygen at standard temperature occupies 710 mL. At what temperature will

it occupy 1000.0 mL if the pressure remains the same?

3) A scientist collected a 24.9 mL sample of carbon dioxide gas at 23°C. What volume will

the gas occupy at standard temperature? Assume the pressure remains constant.

4) A sample of carbon monoxide occupies 3.20 L at 125°C. Calculate the temperature at

which the gas occupies 1.54 L if the pressure is held constant.

5) A quantity of 36.4 L of methane gas is heated from 25°C to 88°C at constant pressure.

What is its final volume?

Chemistry Name __________________________

Hour _______

Assignment 13.1c – Avogadro’s Law Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) A 1.50 mole sample of helium at 25ºC and 1.00 atm pressure has a volume of 31.4 L. A

second sample of helium at the same temperature and pressure has a volume of 42.4 L.

How many moles of helium are in the second sample?

2) Two samples of gas are at the same temperature and pressure. The first sample occupies a

volume of 2.00 L and contains 0.0620 mol of gas. The second sample contains 1.840 mol

of gas. What is the volume of the second sample?

3) Exactly 1.000 mole of gas occupies 22.4 L at 0ºC and 1 atm. What volume will be

occupied by 7.20 mole of gas at the same temperature and pressure?

4) A 10.0 mole sample of oxygen gas occupies 1300 L. How many moles of oxygen would

be in a 2.00 L bottle assuming constant temperature and pressure?

5) On the first breath of air a student blows 0.450 moles of air into a balloon and inflates it

to a volume of 0.180 L. On the second breath the student adds an additional 0.370 moles

of air. What is the new volume of the balloon?

Chemistry Name __________________________

Hour _______

Assignment 13.2a – Ideal Gas Law Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) How much pressure is exerted by 3.40 moles of gas in a 5.00 L bottle at 20.0ºC?

2) What volume is needed to contain 0.550 moles of gas at 1.25 atm and 25.0ºC?

3) How many moles of gas will exert 2.00 atm of pressure in a 2.00 L bottle at 100.0ºC?

4) At what Kelvin temperature will .0750 moles of gas exert 0.980 atm of pressure in a 1.00

L flask?

5) 2.00 moles of gas exerts 720 Torr at 250 K. What volume does the gas occupy?

Chemistry Name __________________________

Hour _______

Assignment 13.2b – Dalton’s Law Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) A 425 mL sample of oxygen is collected over water at 20°C. The sample exerts 750.0

torr of pressure. What volume will the dry gas occupy at standard pressure and 20°C?

2) Chlorine gas can be generated by the reaction of concentrated hydrochloric acid and

potassium permanganate. In order to control the gas it is usually bubbled through water

and collected in an inverted flask. A sample occupying 808 mL at 30°C and 740.0 torr

was collected. What volume will the dry gas occupy at standard pressure? Assume

constant temperature.

3) 450 mL of oxygen is bubbled through water at 10°C and exerts 720.0 torr. What volume

will the dry gas occupy at 730.0 torr and 10°C?

4) At 10°C a gas collected over water exerts 326.3 torr when contained in a 250 mL flask.

What pressure the dry gas will exert if it is transferred to a 100.0 mL flask? The

temperature remains unchanged.

5) What volume would be occupied by a dry gas at 732 torr if the original sample were

collected over water in a 0.250 L flask at 20°C and 842 torr? Assume constant

temperature.

Chemistry Name __________________________

Hour _______

Assignment 13.2c – Gas Stoichiometry Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) What volume of carbon dioxide (at STP) is produced when 14.7 g of coke (carbon) is

burned in air?

C + O2 CO2

2) What volume of chlorine gas (at STP) is needed to produce 74.8 g sodium chloride upon

reaction with excess sodium metal?

2 Na + Cl2 2 NaCl

3) How many mL of chlorine gas are required to produce 50.0 mL of hydrogen chloride

gas? (All measured at STP of course.)

H2 + Cl2 2 HCl

4) When potassium chlorate is heated strongly it decomposes to evolve oxygen gas. How

many grams of potassium chlorate are needed to produce 62.7 liters of oxygen gas at

STP?

2 KClO3 2 KCl + 3 O2

5) What volume of hydrogen cyanide gas (at STP) is produced when 400.0 g of sodium

cyanide react completely with excess sulfuric acid?

2 NaCN + H2SO4 2 HCN + Na2SO4

Chemistry Name __________________________

Hour _______

Assignment 13.3 – Using a Model to Describe Gases

1. When do real gases behave like ideal gases?

2. When does the behavior of a real gas deviate from that of an ideal gas?

3. What are the main ideas of the kinetic molecular theory?

4. Use the kinetic molecular theory to explain Avogadro’s Law.

Chemistry Name __________________________

Hour _______

Assignment 13.4 – Chapter Review (5 pages)

Solve each of the following problems. In order to receive full credit you must do three things: (1)



1) Convert the following pressures into units of atmospheres.

A) 105.2 kPa

B) 767 torr

2) Convert the following pressures into units of mm Hg.

A) 0.9975 atm

B) 99.7 kPa

3) Convert the following pressures into kilopascals.

A) 774 torr

B) 0.965 atm

4) For each of the following sets of pressure and volume data, calculate the missing

quantity. Assume that the temperature and the amount of gas remain constant.

A) V = 53.2 mL at 785 mm Hg; V = ? at 700. mm Hg

B) V = 2.25 L at 1.67 atm; V = 2.00 L at ? atm

C) V = 5.62 L at 695 torr; V = ? at 1.51 atm

5) What pressure (in atmospheres) is required to compress 1.00 L of gas at 760. mm Hg

pressure to a volume of 50.0 mL?

6) What is meant by the absolute zero of temperature? (I want a sentence, not a number.)

7) For each of the following sets of volume and temperature data, calculate the missing

quantity. Assume that the pressure and the mass of gas remain constant.

A) V = 25.0 L at 0°C; V = 50.0 L at ?K

B) V = 247 mL at 25°C; V = 255 mL at ?K

C) V = 1.00 mL at 2272°C; V = ? at 25°C

Chemistry Name __________________________

Hour _______

8) If 0.214 mol of argon gas occupies a volume of 652 mL at a particular temperature and

pressure, what volume would 0.375 mol of argon occupy under the same conditions?

9) If 46.2 g of oxygen gas occupies a volume of 100. L at a particular temperature and

pressure, what volume will 5.00 g of oxygen gas occupy under the same conditions?

10) Given each of the following sets of values for an ideal gas, calculate the unknown

quantity.

A) P = 1.03 atm, V = ?, n = 0.210 mol, T = 27°C.

B) P = ? atm, V = 644 mL, n = 0.092 mol, T = 303 K

C) P = 0.980 atm, V = 11.2 L, n = 0.401 mol, T = ? K

11) What volume does 0.150 mol of nitrogen gas occupy at 58.2°C and 2.04 atm?

12) A tank contains a mixture of 3.0 mol N2, 2.0 mol O2, and 1.0 mol CO2 at 25°C and a total

pressure of 10.0 atm. Calculate the partial pressure of each gas in the mixture.

13) A sample of oxygen gas is saturated with water vapor at 27°C. The total pressure of the

mixture is 772 torr, and the vapor pressure of water is 26.7 torr at 27°C. What is the

partial pressure of the oxygen gas?

14) Consider the following unbalanced chemical equation for the combustion of propane.

______ C3H8 (g) + ______ O2 (g) ______ CO2 (g) + ______ H2O (l)

What volume of oxygen gas at STP is needed for the complete combustion of 5.53 g of

propane?

Chemistry Name __________________________

Hour _______

15) When water is added to magnesium nitride, ammonia gas is produced when the mixture

is heated.

Mg3N2 (s) + 3 H2O (l) 3 MgO (s) + 2 NH3 (g)

If 10.3 g of magnesium nitride is treated with water, what volume of ammonia gas would

be collected at STP?

16) What volume does a mixture of 14.2 g of He and 21.6 g H2 occupy at 28°C and 0.985

atm?

17) What do we assume about the volume of the actual molecule themselves in a sample of

gas compared to the bulk volume of the gas overall? Why?

chapter 13 gases day plans for the day...

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