Honors Chemistry – Chapter 13 and 14 Review Packet
Name: _____________________________
Chapter 13: States of Matter
Section 1: The Nature of Gases
1. What are the three assumptions of kinetic molecular theory?
2. What causes pressure?
3. What is the relationship between kinetic energy and temperature?
Section 2: The Nature of Liquids
1. What is the difference between the particles in a liquid vs. the particles in a solid?
2. Why does evaporation tend to occur at higher temperatures?
3. What is the relationship between the rate of evaporation and the rate of condensation in a closed system
under conditions of dynamic equilibrium?
Section 3: The Nature of Solids
1. What is the structure of most solids?
2. What is a unit cell?
3. What is an allotrope? What is an example of an allotrope?
4. What is an amorphous solid?
Section 4: Changes of State
1. Circle the phase changes that will lead to an increase in energy.
Melting
Evaporation
Deposition
Condensation
Sublimation
Solidification
Honors Chemistry – Chapter 13 and 14 Review Packet
2. Complete the phase change chart:
Starting Phase
Solid
Name: _____________________________
Ending Phase
Liquid
Phase Change
Evaporation
Sublimation
Gas
Liquid
Solid
Solid
Condensation
3. What is the major difference between the phase diagram of water in comparison to other phase
diagrams?
4. Answer the following questions about the phase diagram below:
a. What phase is the compound in:
i. At 70 atm and 200C? ________________________
ii. At 700C and 20 atm? ________________________
iii. At 500C and 80 atm? ________________________
iv. At 60 atm and 400C? ________________________
b. What phase change(s) would occur under the following conditions:
i. The substance at 100C changes from 20 atm to 40 atm ________________________
ii. The substance at 80 atm changes from 300C to 600C ________________________
iii. The substance at 70 atm changes from 200C to 800C ________________________
iv. The substance at 90 atm and 400C drops to 50 atm ________________________
c. On the diagram:
i. Circle the triple point.
ii. Draw a triangle around the critical point.
d. Is it possible to use this phase diagram to determine the normal boiling point of the substance?
Why or why not?
Honors Chemistry – Chapter 13 and 14 Review Packet
Name: _____________________________
Chapter 14: The Behavior of Gases
Section 1: Properties of Gases
1. Complete the following conversions:
a. 90 atm to kPa ________________________
b. 40 C to K ________________________
c. 1800 mmHg to atm ________________________
d. 8675.3 kPa to atm ________________________
e. 498 K to C ________________________
f. 0C to K ________________________
g. 13.2 kPa to mmHg ________________________
h. 400 Torr to atm ________________________
2. Circle the term to best complete each statement:
a. As volume increases, pressure…
increases / decreases
b. As temperature increases, pressure…
increases / decreases
c. As pressure decreases, volume…
increases / decreases
d. As temperature increases, volume… increases / decreases
e. As amount of gas increases, pressure…
increases / decreases
f. As the number of particle collisions decreases, pressure… increases / decreases
Sections 2 and 3: Gas Laws
1. What are the values for STP? ___________________ and ___________________
2. Complete the gas law chart:
Name of Gas Law
Boyle’s Law
Equation
Value Held Constant Required Units (If necessary)
Same on both sides
V1/T1 = V2/T2
Gay-Lussac’s Law
Temperature in Kelvin
Combined Gas Law
N/A
PV = nRT
Ptotal = P1 + P2 + …
Graham’s Law
All same pressure units
N/A
3. Sample problems for each gas law:
a. Boyle – If 85.2 L of nitrogen at 0.750 atm are compressed to 760 mmHg at constant temperature,
determine the final volume of nitrogen.
Honors Chemistry – Chapter 13 and 14 Review Packet
Name: _____________________________
b. Charles – 9.50 L of oxygen gas is compressed to 4.75 L. The initial temperature is 17.0C.
Calculate the final temperature of the oxygen gas.
c. Gay-Lussac – A constant volume of gas is pressurized from 2.0 atm to 13.0 atm. The original
temperature is 5.0C. Calculate the final temperature.
d. Combined Gas Law – A gas balloon has a volume of 652.0 L when the temperature is 45.0C
and the pressure is 730.0 mmHg. What will the new volume be when the temperature is 21.0C
and 770.0 mmHg?
e. Ideal Gas Law – How many moles of xenon are contained in a 1.250 L container at 21.0C and
0.986 atm?
f. Dalton’s Law – If a mixture of gases made up of ammonia, sulfur dioxide (PSO2 = 25.66 mmHg),
and carbon monoxide (PCO2 = 74.98 mmHg) has a total pressure of 150 mmHg, calculate the
partial pressure of ammonia.
g. Graham’s Law – If neon travels at 400 m/s at a given temperature, calculate the rate of diffusion
of butane (C4H10) at the same temperature.
4. Solve the following problems. First decide which law you must use (write the name of the law on the
line) and then solve. Be sure to include units on all answers.
a. ___________________ - Calculate the pressure of 85.4 g of oxygen gas in a 3.00 L container at
24C.
Honors Chemistry – Chapter 13 and 14 Review Packet
Name: _____________________________
b. ___________________ - A pressure of 800 kPa is required to inflate a balloon to a volume of
225.0 mL. What is the final pressure when the balloon reaches its maximum volume of 1.2 L?
c. ___________________ - A balloon is filled to a pressure of 1130 kPa inside a party store. After
you take it outside, where the temperature is 273 K, the pressure decreases to 1003 kPa. What
was the temperature inside the store (in Celsius)?
d. ___________________ - A gas has a volume of 5.2 L at 45.5C. What is the volume at 32C?
e. ___________________ - A soda can is taken from a cooler at a temperature of 5C and a
pressure of 2.01 atm. The can warms to a temperature of 21C. What is the final pressure?
f. ___________________ - If 240 mL of air at standard pressure is compressed to a pressure of
0.85 atm, what will the compressed volume of gas be?
g. ___________________ - You buy a 250 mL bag of chips at an airport where the air pressure is
1.03 atm. After take-off, the pressure in the plane has decreased to 0.76 atm and the temperature
is 19C. You notice that the bag has increased in volume to 341 mL. What was the temperature
inside the airport?
h. ___________________ - How many moles of oxygen gas are in a tank that is 30.0 L if the
temperature is 300 K and the pressure is 207.5 kPa?
Honors Chemistry – Chapter 13 and 14 Review Packet
Name: _____________________________
i. ___________________ - A nitrogen molecule has a rate of diffusion of 505 m/s at room
temperature. What is the rate of diffusion of helium at the same temperature?
j. ___________________ - The pressure of a gas is reduced from 214.2 kPa to 330.0 mmHg as the
volume is increased from 95.0 mL to 850 mL. What would the final temperature be if the
original temperature was 65.0C?
k. ___________________ - Helium diffuses 10 times faster than an unknown gas. Find the molar
mass of the unknown gas.
l. ___________________ - Determine the total pressure of a mixture of gases containing 10 moles
of NH3, 2 moles of CO, and 15 moles of SO2 at a temperature of 41°C in a volume of 21 L.
m. ___________________ - At what temperature would a gas whose volume is 250.0 mL at 72C
double its volume?
n. ___________________ - A helium balloon is fully inflated to 0.9 L in a store where the pressure
is measured at 5.7 kPa and the temperature in the store is 24C. The balloon is taken outside,
where the pressure is 4.8 kPa. The balloons volume increases to 1.0 L and the balloon explodes!
What is the temperature outside (in Celsius)?
o. ___________________ - I have an unknown volume of gas at a temperature of 115 K in a
container with a pressure of 60 atm. If by increasing the temperature to 225 K and decreasing
the pressure to 30 atm causes the volume of the gas to be 29 L, how many L of gas did I start
with?