Download Kinetic-Molecular theory of Matter/Ch10, Gases/Ch11 –Column

Kinetic-Molecular theory of Matter/Ch10, Gases/Ch11 –Column notes: Answer all parts of each question IN
YOUR OWN WORDS. Use the text, figures and captions as resources.
Section 10-1: The Kinetic-Molecular Theory of Matter
1) How does the word kinetic apply to
particles of matter?
2) Briefly describe the postulates of the
Kinetic Molecular Theory (KMT).
3) What is the relationship between
temperature and average kinetic energy?
4) What is the mathematical relationship
between average kinetic energy and
velocity of particles? Therefore, what is
the relationship between temperature
and velocity?
5) Using the KE equation, explain why
balloons filled with helium (molar mass
4g/mol) deflate faster than those filled
with air (molar mass 29g/mol)
6) What is an ideal gas? Do any actually
exist? Why do we care about them?
7) Describe the properties of gases and
how each can be explained by the KMT?
8) Which postulates of KMT do real gases
not follow? What types of gases are
most like ideal gases? What types of
gases are most like real gases?
11-1 Gases and Pressure
9) What causes pressure? How is it defined
(include units)? Why does the pressure
on your feet change if you are on tip
toes?
10) What gas characteristics does pressure
depend on?
11) What causes atmospheric pressure?
What is the value for this pressure at sea
level (including units)? Write the
equivalent pressures in atmospheres,
pascals, millimeters of mercury, torr,
kilopascals, and pounds per square inch.
12) What is standard temperature and
pressure? Why do scientists want these
variables standardized for gas
measurements?
13) Describe how a barometer measures
atmospheric pressure.
14) Describe how a manometer measures
the pressure inside a closed container.
15)
The pressure of oxygen on Mount
Everest is 47.88 mmHg on a given
day(your lungs need about 100 mmHg
oxygen for you to survive). Using
conversion factors, calculate this mountain
pressure in units of atmospheres, pascals,
torr, kilopascals, and pounds per square
inch. (see sample problem A)
16) What is Daltons law of Partial Pressure?
How is it related to the KMT?
17) Calculate the partial pressure, in mmHg,
exerted by the 4 main gases in air at
760mmHg if the abundance of nitrogen is
78.08%, oxygen 20.95%, argon 0.934%,
carbon dioxide 0.035%. Show work.
18) Based on Figure 5 on p366, when gases
are generated in a chemical reaction,
why is it convenient to collect them by
water displacement? Why do you have
to correct the total atmospheric
pressure in order to determine the
accurate pressure of the gas from the
reaction?
19) After reading the Chemistry in Action
article, answer the following questions:
a) Explain how increased water
pressure can cause nitrogen narcosis
in scuba divers (an intoxicating
feeling)
b) Explain how Henry’s Law can cause
decompression sickness (“the
bends”) if a diver comes up too
quickly.
11-2 The Gas Laws
20) What are the 4 variables of gases?
21) What two variables are related in Boyle’s
Law? What is the equation used for this
relationship? Are the 2 variables directly
or inversely related and explain how you
know this? What 2 variables must be kept
constant?
22) How is Boyles Law related to the KMT?
23) Do the practice problem on p370. Show
work.
24) What two variables are related in Charles’
Law? What is the equation used for this
relationship? Are the 2 variables directly
or inversely related and explain how you
know this? What 2 variables must be kept
constant?
25) What units of temperature must be used
for this calculation? How do you convert
from one unit to the other?
26) How is Charles Law related to the KMT?
27) Do practice problem 1 on p372. Show
work.
28) What two variables are related in GayLussac’s Law? What is the equation used
for this relationship? Are the 2 variables
directly or inversely related? What 2
variables must be kept constant?
29) What does “Combined” mean in the
Combined Gas Law. Demonstrate how
each of the 3 previous gas laws can be
obtained from the Combined Gas Law.
30) If 5 out of 6 of the Combined Gas Law
variables are known, the 6th can be solved
for. Do Practice Problem 1 on p375.
11-3 Gas Volumes and the Ideal Gas Law
31) What does Avogadro’s Law tell us about
the number of gas molecules and the
volume they occupy? What 2 variables
must be kept constant?
32) How can coefficients of a balanced
equation involving gases be used to
determine the ratio of the volumes.
33) How many molecules are contained in
22.4 liters of a gas at STP? What is this
volume called?
34) How does mass of a molecule affect its
volume?
35) Do Practice Problems 1 and 2 on p381.
36) How can Avogadro’s relationship
between volume and moles be used to
do stoichiometry calculations.
37) Do Practice Problem 2 on p382.
38) How does the ideal gas law relate the 4
gas variables? Do any of them need to
be kept constant for this relationship to
work?
39) What does R represent in the Ideal Gas
Law? How were the number and its
units derived from the other 4
quantities?
40) Why are there 4 different numbers for
the gas constant R? How do you decide
which one to use for a particular
problem? Which units will you usually
use for volume, pressure, temperature
and amount?
41) Do Section Review problem 5 on p385.
Make sure to check units and convert
those which will not fit with R units.
11-4 Diffusion and Effusion
42) Compare and contrast Diffusion and
Effusion.
43) How is Kinetic Energy related to the
mass of a molecule? To the velocity of a
molecule?
44) What postulate in the KMT is used to
derive Grahams Law of Effusion. What is
the equation for this Law?
45) Calculate the molar mass of a gas that
effuses at 1.6 times faster than carbon
1.6
dioxide. (hint: set the ratio as 1 and
identify which of these will be the larger
molecule and which will be the smaller
one). Use sample problem to guide you.