HW 1 Gas Properties After Reading Lesson 131 Answer

hw #1 gas properties after reading lesson 13.1, answer the following questions. kinetic theory and a model for gases 1. the energy an

HW #1 Gas Properties
After reading Lesson 13.1, answer the following questions.
Kinetic Theory and a Model for Gases
1. The energy an object has because of its motion is called KINETIC .
2. Circle the letter of each sentence that is true about the
assumptions of the kinetic theory
concerning gases.
a. A gas is composed of particles with insignificant volume that are
relatively far apart.
b. Strong attractive forces exist between particles of a gas.
c. Gases tend to collect near the bottom of a container.
d. The paths of uninterrupted travel of particles in a gas are
relatively short because the
particles are constantly colliding with each other or with other
objects.
3. Is the following statement true or false? According to the kinetic
theory, collisions
between particles in a gas are perfectly elastic because kinetic
energy is transferred
without loss from one particle to another, and the total kinetic
energy remains constant. _TRUE_______
Gas Pressure
4. Gas pressure results from the force exerted by a gas per UNIT
SURFACE AREA OF AN OBJECT.
5. Simultaneous collisions of billions of particles in a gas with an
object result in GAS PRESSURE.
6. What force holds the particles of air in Earth’s atmosphere?
GRAVITY
7. What kind of pressure is measured with a barometer? ATMOSPHERIC
PRESSURE
8. Circle the letter next to every name of a unit of pressure.
a. mm Hg
d. kPa
b. standard
e. atm
c. pascal
f. degree
9. Standard temperature and pressure (STP) are defined as
TEMPERATURE OF O°C
PRESSURE OF 1atm or 101.3kPa, or 760 mmHg
Kinetic Energy and Temperature
10. What happens to the temperature of a substance when the average
kinetic energy of its
particles increases?
THE TEMPERATURE OF THE SUBSTANCE INCREASES
11. Is the following statement true or false? All the particles in a
substance at a given
temperature have the same kinetic energy. FALSE
12. The temperature 0 K, or −273.15°C, is called ABSOLUTE zero.
Theoretically, particles of matter at this temperature would have no
KINETIC ENERGY.
13. On the graph below, write the labels lower temperature and higher
temperature to
identify the curve that depicts the kinetic energy distribution of
particles in a liquid at a
lower temperature and at a higher temperature.

LOWER TEMP
HIGHER TEMP
14. Circle the letter of the temperature scale that correctly
completes this sentence.
Temperature on the scale is directly proportional to the average
kinetic
energy of the particles of a substance.
a. Celsius
c. Fahrenheit
b. Kelvin
d. Centigrade
Practice converting between different units of pressure.
15. Determine how many mm of Hg are equal to 5.3 atm of pressure.
5.3 atm X760mmHg = 4028 mm Hg
1 atm
16. Determine how many atmospheres of pressure are equal to 65.78 kPa.
65.78 X 1atm= 0.65 atm
101.3 kPa
17. If you have 2.86 atm of pressure, is that more or less than 2000
mm of Hg?
2.86 atm X760 mmHg = 2174 mmHg (> 2000 mm of Hg)
1 atm
18. What is the pressure in both mm of Hg and atmospheres if you are
given 5678.32 Pa?
5678.32 Pa X 1 kPa X 1 atm = 0.0561 atm
1000 Pa 101.3 kPa
5678.32 Pa X 1 kPa X 760 mmHg = 42.60 mmHg
1000 Pa 101.3 kPa
HW #2 Liquids
After reading Lesson 13.2, answer the following questions.
1. Is the following sentence true or false? The kinetic theory states
that there are no
attractions between the particles of a liquid. FALSE
2. Circle the letter next to each sentence that is true about the
particles of a liquid.
a. Most of the particles in a liquid have enough kinetic energy to
escape into a gaseous
state.
b. Liquids are much denser than gases because intermolecular forces
reduce the amount
of space between the particles in a liquid.
c. Increasing pressure on a liquid has almost no effect on its volume.
d. Liquid particles are free to slide past one another.
3. The conversion of a liquid to a gas or vapor is called VAPORIZATION
.
4. When vaporization occurs at the surface of a liquid that is not
boiling, the process is
called EVAPORATION .
5. As a liquid evaporates, why do only some of the particles break
away from the surface of
the liquid? Why does the liquid evaporate faster if the temperature is
increased?
THE PARTICLES THROUGHOUT HAVE DIFFERENT KEs; ONLY SOME HAVE ENOUGH TO
ESCAPE. THE KE OF ALL PARTICLES INCREASES AS TEMP INCREASES, SO MORE
PARTICLES HAVE ENOUGH KE TO ESCAPE.
6. Is the following sentence true or false? Evaporation is a cooling
process because the
particles in a liquid with the highest kinetic energy tend to escape
first, leaving the
remaining particles with a lower average kinetic energy and, thus, a
lower temperature.
TRUE
Questions 7–10 refer to either container A or container B below. Think
of each container as a
system involving both liquid water and water vapor.

7. From which of the containers are water molecules able to escape? B
8. In which container can a dynamic equilibrium be established between
water molecules
in the liquid state and water molecules in the vapor state? A
9. In which container will the water level remain constant? A
10. From which container is it possible for all of the liquid water to
disappear through
evaporation? B
HW # 3 Changes of State
A s you read Lesson 13.4, use the concept map below. On each
arrow, fill in the appropriate
change of state.

solid
4.deposition
1.melting
2.freezing
3.sublimation
5.vaporization
liquid
gas
6.condensation
EXTENSION Give a real-life example of each change of state shown in
the concept map.
1.
Ice changing to liquid, 2) molten steel solidifying, 3) dry ice
changing to CO2, 4)formation of frost from water vapor in the air,
5) a wet cloth drying 6) dew forming on the grass
Sublimation
1. The process by which wet laundry dries on an outdoor clothesline in
winter is called
SUBLIMATION .
2. Is the following sentence true or false? Solids have vapor pressure
because some particles
near the surface of a solid substance have enough kinetic energy to
escape directly into
the vapor phase. TRUE
Phase Diagrams
3. What does a phase diagram show?
A PHASE DIAGRAM SHOWS THE TEMPERRATURE AND PRESSURE CONDITIONS AT
WHICH A SUBSTANCE EXISTS IN THE SOLID, LIQUID , AND VAPOR PHASES
4. What is the triple point of a substance?
THE TRIPLE POINT REPRESENTS THE ONLY CONDITIONS OF TEMPERATURE AND
PRESSURE AT WHICH THREE PHASES OF A SUBSTANCE CAN EXIST IN EQULIBRIUM
5. In the phase diagram for water shown below, label the melting point
and boiling point at
normal atmospheric pressure, and the triple point.

NORMAL BOILING POINT
NORMAL MELTING POINT
TRIPLE POINT
6. Use the phase diagram above to answer the following question. Why
is a laboratory
required to produce the conditions necessary for observing water at
the triple point?
FROM THE DIAGRAM, THE TRIPLE POINT OF WATER IS AT A PRESSURE OF 0.61
kPa,
FAR BELOW ATMOSPHERIC PRESSURE. ONE CAN ONLY OBSERVE WATER AT ITS
TRIPLE POINT WITH LAB EQUIPMENT; LAB EQUIPMENT IS NECESSARY TO ACHIEVE
PRESSURES THIS LOW.
7. Use the diagram on page 10 to determine the relative humidity if
the water vapor pressure is 200mbar at 80°C.
8. According to page 10, which set of conditions below would cause it
to start to rain?
a.
The water vapor pressure rises above 300mbar on a 70°C day.
b.
The water vapor pressure is 400mbar on an 80°C day. A cold front
comes in and the temperature drops to 50°C.
c.
The water vapor pressure is 400mbar on an 80°C day. The
temperature goes up to 90°C the next day, and the pressure does
not change.
HW #4 Phase Diagram Worksheet
Refer to the phase diagram below when answering the questions on this
worksheet:

TRIPLE POINT
Straight Arrow Connector 23
CRITICAL POINT
Straight Arrow Connector 25
SOLID
LIQUID
GAS
Straight Arrow Connector 31 Straight Arrow Connector 32
Straight Arrow Connector 34 Straight Arrow Connector 35
1) Label solid, liquid, gas, the triple point and the critical point
on this diagram. ________
2) What is the normal boiling point of this substance? _350 0 C _
3) What is the normal freezing point of this substance? 100 0 C
4) If I had a quantity of this substance at a pressure of 1.25 atm and
a temperature of 3000 C and lowered the pressure to 0.25 atm, what
phase transition(s) would occur? At what pressure?
VAPORIZATION WOULD OCCUR AT A PRESSURE OF 0.9 atm____________
__________________________________________________________________
5) Can I drink the substance at 0.50atm? NO AT 0.50 atm HE SUBSTANCE
CAN ONLY EXIST AS A SOLID OR GAS________
6) If I had a quantity of this substance at a pressure of 0.75 atm and
a temperature of -1000 C, what phase change(s) would occur if I
increased the temperature to 6000 C? At what temperature(s) would they
occur?
MELTING WOULD OCCUR AT 90 0 C AND VAPORIZATION WOULD OCCUR AT 150 0 C___________________________________________________________________
____________________________________________________________________