CHM 2045C                                    Name: _________________
Module Six Homework Packet

  Module Six: The Gaseous State  (Chapter 9) Assignment Outline

A._____(05) Kinetic Molecular Theory-Section 9.6 Answer  ppt9

B._____(05) Discussion Real vs Ideal Gas Equation-Sect 9.8 Answer bc

C._____(05) Standard Conditions/Molar Volume-Sect 9.1-9.2 Answer bc

D._____(05) Gas Laws/Vocabulary-Sections 9.2-9.3, 9.5, 9.7 Answers

E._____(10) Gas Law Problems-Sections 9.2-9.3, 9.5, 9.7 Answers

F. _____(05) Volume-Volume Stoichiometry Problem-Section 9.4 Answers fg

G._____(05) Mass-Volume Stoichiometry Problem-Section 9.4 Answers fg

H._____(05) Gas Densities/Molecular Mass Determination-Sect 9.4 Answers

I. __ ___(05) Effusion & Diffusion of Gases-Section 9.7 Answers

______(50) Total = ______%


Module Six- Part A: Kinetic Molecular Theory    5 points


 State the 5 assumptions of the Kinetic Molecular theory as stated in the book (Section 9.6) :






















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



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Module Six Part B: Discussion Question   5 points


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



Sections 9.1-9.2



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Module Six Part D Gas Laws                                         05 points




Boyle’s Law (In words and formula)





Charles Law (in words and formula)





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






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






Avogadro’s Law (in words and formula)







Combined Gas Law Equation (write only the equation)





Ideal Gas Equation (write only the equation)





Define Vapor Pressure





Graham’s Law of Diffusion(in words and formula)



Module Six Homework Packet – Page 4

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 5

Part F Volume-Volume  Stoichiometry        5 points


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


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 6

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)














Module Six Part H-2 Molecular Mass Determination Problem 


Calculate the molecular weight of an unknown liquid that when vaporized at 99 oC and 755 torre , gave 125.0 mL of vapor with a mass of 0.673 grams .




















Module Six Homework Packet – Page 7


Module Six Part I Effusion of Gasses Problem                   5 points


A sample of Nitrogen gas escapes through a tiny hole in 44.0 seconds.  An unknown gas escapes under the same conditions in 80.0 seconds.  Calculate the molecular mass of the unknown.