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) :

1

2

3

4

5.

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

Reference:

Sections 9.1-9.2

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Module Six Part D Gas Laws 05 points

State:

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)

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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 27^oC. 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 25^oC 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.