**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**

**Module
Six Homework Packet-Page 2**

**Module Six Part B: Discussion Question 5 points **

In the Real Gas Equation:
(P + an** ^{2}**/V

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 ^{o}**C**** **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

_{ }

_{ }

1 mole** _{ N2 }**=________L

Reference:

Sections
9.1-9.2

**Module
Six Homework Packet Page 3**

**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)

**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 ** ^{o}**C
and

760 mmHg. What volume will the gas occupy at 25 ** ^{o}**C 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 ** ^{o}**C. 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 ** ^{o}**C.
Calculate the pressure in torre if the
temperature is changed to 127

__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 ** ^{o}**C at 760 torre
pressure with the temperature remaining constant. (The partial pressure of water vapor at 25

**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^{o}C.
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^{o}C 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 ** ^{o}**C 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
N _{2}** and

**Part G Mass-Volume Stoichiometry 5 points**

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

** KClO**_{3}** ****à**** KCl + O**_{2}

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***C _{8}H_{18} vapor **at STP?

Calculate the gas density of *octane
gas***C _{8}H_{18} **at

(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 ^{o}C** and

**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