CHM 1025C                                    Name: _________________
Module Six Homework Packet

 Module Six: The Gaseous State  (Chapter 10)

A1._____(12) Properties of Solids (11.4), Liquids(11.1), and Gases 10.1 Answers

A._____(10) Kinetic Molecular Theory-Section 10.10 page299  Answers a

B._____(00) Discussion Real vs Ideal Gas Equation-Sect 10.10 Answer bc

C._____(08) Standard Conditions/Molar Volume-Sect 8.5 Answer bc

D._____(10) Gas Laws/Vocabulary-Sections 10.4, 10.5, 10.6, 10.7, 10.8, 10.9 Answers

E._____(30) Gas Law Problems- Sections 10.4, 10.5, 10.6, 10.7, 10.8, 10.9, 10.10 Answers

F. ____ (10) Volume-Volume Stoichiometry Problem-Section 9.6 Answers fg

G._____(10) Mass-Volume Stoichiometry Problem-Section 9.5 Answers fg

H._____(10) Density (STP & Other Conditions) Section 8.5/10.10 Answers

______(100) Total = ______%

M._____(100) Multiple Choice Exam Chapter 10
M-6 Required Homework:

   ______(50) M-6 Pretest Hardcopy Homework Packet

   ______(50) M-6 Multiple Choice (MC) Practice (Chapter 10 only) (Blackboard Online)

Module Six- Part A: Kinetic Molecular Theory    5 points


 State the 5 assumptions of the Kinetic Molecular theory as stated in the book (Section 11.10 pages 300-1) :






















For shorter answers reference section 10.10 page 299-300 and write only the bold black sentences

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Module 6 A Properties of Solids, Liquids and Gases  5 Points


State four of the five properties of solids (Section 13.4 Corwin Text):












State four of the five properties of liquids (Section 13.1 Corwin Text):












State four of the five properties of gases (Section 11.1 Corwin Text):













Properties of Gases: Section 10.1 page 280

Properties of Liquids: Section 11.1 page 312

Properties of Solids: Section 11.4 Pages 319-320



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Module Six Part B: Discussion Question (up to 5 points bonus)


In the Real Gas Equation:   (P + an2/V2) (V - nb) = n RT a pressure correction factor was added. Why? (What assumptions of the kinetic theory breakdown under extreme conditions of temperature and pressure?)











Also a volume correction factor was subtracted. Why? (What assumptions of the KMT breakdown under extreme conditions?)









Module Six-Part C    Standard Conditions/Molar Volume     5 points


State standard conditions (STP) in three units of pressure (the last is your choice) and oC and K temperatures:



_____mm Hg or ______torre=  ______atm =  _____   ______(you write the unit too)



_____ oC   =    ______K


Are the values for the Molar Gas Volume Constant:


1 mole CO2 =________L CO2@STP       1 mole H2 =________L H2@STP



1 mole N2 =________L N2@STP            1 mole O2 =________L O2@STP



Standard Temperature: See Section 8.5 page 231

STP: See Section 10.8 Page 294

Units of Pressure/Standard Pressure: Section 10.2 See Table 10.1 p282

Molar Volume Constant: Section 8.5 Pages 230-233 See Table 8.1 page 231

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Module Six Part D Gas Laws                                         10 points




Boyle’s Law (In words and formula) (See Section 10.4)





Charles Law (in words and formula) (See Section 10.5)





Dalton’s Law of Partial pressures (in words and formula) (See Section 10.9)






Gay-Lussac’s Law (in words and formula) (See Section 10.6)






Avogadro’s Law (in words and formula) (see Section 8.5 p 230, Section 9.1 page 250)







Combined Gas Law Equation (write only the equation) (See Section 10.7):





Ideal Gas Equation (write only the equation) (See Sections 10.10 and 10.11)





Define Vapor Pressure (See Section 10.8):





Bonus: Graham’s Law of Diffusion


Module Six Homework Packet – Page 5

Module Six Part E Gas Law Problems                            10 points

Boyle’s Law (See Section 10.4 and Example 10.3) (Additional Problems p307-8 #15-20)

1.  A sample of a gas has a volume of 100 mL when measured at 25 oC and

 760 mmHg.  What volume will the gas occupy at 25 oC and 380 mmHg?




Charles Law(See Section 10.5 and Example 10.4) (Additional Problems p308 #21-26)

2. The volume of a gas is 100.0 mL at 27 oC.  At what temperature in degrees Celsius would the volume of the gas be 200.0 mL, assuming the pressure remains constant.





Gay-Lussac’s Law (See Section 10.6 and Example 10.5) (Additional Problems p308 #27-32)

3.  A sample of gas occupies 100.0 L at 710.0 torre and 27 oC.  Calculate the pressure in torre if the temperature is changed to 127 oC while the volume remains constant.





Dalton’s Law of Partial Pressures (See Section 10.4 & Example 10.3) (Additional Problems p307-8 #15-20)

4. Calculate the dry volume in milliliters of 200 mL of hydrogen gas collected over water at 25 oC at 760 torre pressure with the temperature remaining constant.  (The partial pressure of water vapor at 25 oC is 23.8 torre.)




Avogadro’s Law (See Pages 230, 250, and 271)

5.   A 1.5 mole sample of a gas occupies 25.0 L at 758 torre and 27oC. Calculate the Volume of the gas, if more molecules are injected into the vessel increasing the moles to 2.5 moles, provided the pressure and the temperature do not change.




Combined Gas Laws (See Section 10.7 and Example 10.6) (Additional Problems p308 #33-42)

6. A100.0 mL sample of air is collected at 25oC and 774 mmHg. What is the volume at STP?






Ideal Gas Equation (See Section 10.11) (Additional Problems p308 #63-66)

7. Calculate the number of moles of nitrogen gas in a 5.00 L cylinder at 27 oC and 4 atm pressure. R = 0.0821 L atm/ K mole )





How much does this volume of gas weigh?




Module Six Homework Packet – Page 6

Part F Volume-Volume  Stoichiometry        5 points

(See Section 9.6 and Example 9.8) (Additional Problems p275 #37-48)


In the Haber process, nitrogen N2 and hydrogen H2 gases combine to give ammonia gas NH3 as the only product. If 5.55 L of nitrogen gas completely reacts, calculate the volume of ammonia that is produced. Assume all volumes of gas are measured under constant conditions of 500 oC and 300 atm pressure. How many liters of hydrogen are required to complete react the 5.55L of nitrogen?
















Part G Mass-Volume  Stoichiometry       5 points

(See Section 9.5 and Examples 9.6 and 9.7) (Additional Problems p274-5 #29-36)


Potassium chlorate is used in the lab to make oxygen gas by the following (unbalanced) reaction:

                           KClO3      à        KCl        +        O2

How liters of oxygen may be made from reacting  1.226 grams of Potassium chlorate?











Module Six Homework Packet – Page 7

(See Section 8.5 and Example 8.8) (Additional Problems p245 #25-30)

Module Six Part H-1 Gas Density Problem                   5 points

Calculate the gas density of octane gas C8H18 vapor at STP?










Calculate the gas density of octane gas C8H18 at 27 oC and 750 torre?.

(Hint calculate the volume using the ideal gas equation)