Transcript Slide 1

Chemistry 177
November 20, 2009
Take out CLICKERS:
“GO 41 GO” -or- “CH 41 CH” and CALCULATORS
NEXT LECTURE:
Monday, Nov. 30; Bring CLICKERS
READ BLBM, Chapter 10
HOMEWORK #15:
Ch. 10: # 32, 36, 44, 54, 58, 66
Due in Recitation, Thursday December 3
OPTIONAL EXAM:
Monday, December 7, 6:30-7:30 PM (Multiple Choice)
FINAL EXAM:
Monday, December 14, 7-9 PM
Have a restful Thanksgiving break
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Chapter 10: Gases
Avogadros’ Law
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Chapter 10: Gases
Avogadro's Hypothesis
Gay-Lussac's Law of Combining Gas Volumes
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Chapter 10: Gases
Ammonia burns in oxygen to form nitric oxide
(NO) and water vapor. How many volumes of
NO are obtained from one volume of ammonia
at the same temperature and pressure?
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Chapter 10: Gases
Clicker Question
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Chapter 10: Gases
Ideal Gas Equation (“Law”)
Boyle’s law:
Charles’ law:
Avogadro’s law:
 2009, Prentice-Hall, Inc.
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Chapter 10: Gases
Argon is an inert gas used in lightbulbs to retard the
vaporization of the filament. A certain lightbulb
containing argon at 1.20 atm and 18 0C is heated to
85 0C at constant volume. What is the final pressure of
argon in the lightbulb (in atm)?
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Chapter 10: Gases
The conditions 0 0C and 1 atm are called standard
temperature and pressure (STP).
Experiments show that at STP, 1 mole of an ideal
gas occupies 22.414 L.
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Chapter 10: Gases
What is the volume (in liters) occupied by 49.8 g of HCl
at STP?
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Chapter 10: Gases
Clicker Question
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Chapter 10: Gases
Density (d) Calculations
PM
m
d=
=
V
RT
Molar Mass (M ) of a Gaseous Substance
dRT
M=
P
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Chapter 10: Gases
A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm
and 27.0 0C. What is the molar mass of the gas?
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Gas Stoichiometry
Chapter 10: Gases
Some automobile airbags use the decomposition of
sodium azide, NaN3(s), into Na(s) and N2(g) to inflate
the bag in an accident. A typical charge of NaN3(s) is
60.0 g. Estimate the volume of the airbag when this
charge completely decomposes at 1.00 atm and 298.0 K
NaN3 (s)
Na(s) + 3/2 N2(g)
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Chapter 10: Gases
Dalton’s Law of Partial Pressures
V and T
are
constant
P1
P2
Ptotal = P1 + P2
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Chapter 10: Gases
Consider a case in which two gases, A and B, are in a
container of volume V.
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Chapter 10: Gases
A sample of natural gas contains 8.24 moles of CH4,
0.421 moles of C2H6, and 0.116 moles of C3H8. If the
total pressure of the gases is 1.37 atm, what is the
partial pressure of propane (C3H8)?
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Chapter 10: Gases
Clicker Question
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