1 Unit 10: Gas Laws Name: Class Period: Test Date: February 25th Monday Tuesday Wednesday Thursday Friday February 8 Stoichiometry Test Review 9 Stoichiometry Test 10 Review for Cumulative Retest 11 Cumulative Re-Test 12 Pressure & Kinetic Theory of Gases HW: p.4 Bring an empty soda can to class monday 15 Combined Gas Law Soda can activity HW: p.8 16 Boyle’s, Charles’, and Avogadro’s Law- HW: pp.14 – 15 17 Chem Think Gas Laws Tutorial- Computer Lab- 18 Gas Laws Lab/Activity Begin working on Study Guide- pgs. 24-28 Study for Quiz on Friday 19 Quiz Dalton’s Law of Partial Pressures HW: Pg. 17 Study Guide- pgs. 24-28 22 Ideal Gas Law HW: p.20 Study Guide- pgs. 24-28 23 Stoichiometry with Gas Laws HW: p.23 and study guide (pp.24-28) 24 Review for Test Study Guide Due TODAY!! 25 Gas Laws Test 26
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1
Unit 10: Gas Laws Name:
Class Period: Test Date: February 25th
Monday Tuesday Wednesday Thursday Friday
February 8 Stoichiometry Test Review
9 Stoichiometry Test
10 Review for Cumulative Retest
11 Cumulative Re-Test
12 Pressure & Kinetic Theory of Gases HW: p.4 Bring an empty soda can to class monday
15 Combined Gas Law Soda can activity HW: p.8
16 Boyle’s, Charles’, and Avogadro’s Law- HW: pp.14 – 15
17 Chem Think Gas Laws Tutorial- Computer Lab-
18 Gas Laws Lab/Activity Begin working on Study Guide- pgs. 24-28 Study for Quiz on Friday
19
Quiz Dalton’s Law of Partial Pressures HW: Pg. 17 Study Guide- pgs. 24-28
22 Ideal Gas Law HW: p.20 Study Guide- pgs. 24-28
23 Stoichiometry with Gas Laws HW: p.23 and study guide (pp.24-28)
24 Review for Test Study Guide Due TODAY!!
25
Gas Laws Test
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2
Pressure
1. What is the definition of pressure?
2. What causes pressure?
3. Which shoes create the most pressure? How does changing the area of contact affect the amount of pressure
exerted by an object?
4. What are the units used to measure pressure?
5. How do I convert between units of pressure?
atm = mmHg = kPa = psi
6. How many kilopascals are equivalent to 880 mmHg?
7. Calculate the number of pounds per square inch (psi) that are in 2.60atm.
Temperature – ALWAYS use absolute temperature (Kelvin) when working with gases.
Conversion:
K = °C + 273
Practice problems:
32°C = __________ K How much is 75°C in Kelvin?
3
The Behavior of Gases and the Kinetic Theory
Kinetic refers to __________________.
The energy an object has, because of its motion, is called __________________________
The Kinetic theory states that “the tiny particles in all forms of matter are in
______________________________.”
Watch the video segment (Kinetic Molecular Theory in the video Standard Deviants School Chemistry:
Molecular Geometry) on Discovery Education and fill in the missing information
A. What happens when a closed container is inflated?
B. A gas inside a bicycle tire exerts a pressure of 35 pounds per square inch (psi). How much air must be
pumped into the tire to produce a pressure of 70 psi?
** The relationship between amount of gas and pressure is proportional, assuming the volume & temperature
stay the same.
C. What happens to pressure when a closed container is deflated?
(Note: Gas particles move from region of higher pressure to lower pressure until equilibrium is reached.)
HOMEWORK Day 1 - Practice Problems on Pressure & Temperature Conversions Show all work! Record your answer with the correct number of significant figures and units!
1. Calculate the pressure of 1.3atm in mmHg.
2. Convert 56kPa to psi.
3. How many atmospheres are equivalent to 230kPa?
4. What is 560K on the Celsius scale?
5. Water boils at 100oC. What is the boiling point of water in Kelvin?
5
COMBINED GAS LAW
The Combined Gas Law helps us explain what happens to gases as the pressure, temperature, and volume changes in
respect to moles of a substance.
Letter or
Number Variable Name Unit Conversions
P
V
6
Letter or
Number Variable Name Unit Conversions
n*
T
1
2
*NOTE: If “n” is not given in a problem, assume it to be 1 mole.
Temperature must be in .
Remember: STP = ____ atm and ________ K or ____°C
Guided Practice:
1. A hot air balloon has a volume of 7500L at 270K and a pressure of 1.2 atm. What will be the volume of the
balloon if the pressure changed to 0.90atm and the temperature decreases to 230K?
Givens and Unknowns:
P1 =
V1 =
n1 =
T1 =
P2 =
V2 = unknown
n2 =
T2 =
Equation:
Substitute & Solve:
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2. The volume of a gas at STP is 22.4L. At 12oC, the volume of the balloon changes to 55.0L. What is the new
pressure?
Givens and Unknowns:
P1 =
V1 =
n1 =
T1 =
P2 =
V2 =
n2 =
T2 =
Equation:
Substitute & Solve:
=
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Homework - Combined Gas Law Practice
1. A 5.00 L air sample at 170 K has a pressure of 107 kPa. What is the new pressure if the temperature is
raised to 548 K and the volume expands to 7.00L?
2. A gas at 880mmHg and 298K occupies a container with an initial volume of 1.00 L. The pressure increases to
1980mmHg as the temperature rises to 398K. What will be the new volume?
3. The volume in a gas filled balloon is 30.0 L at 40°C and 3.6 atm of pressure. What volume will the balloon
occupy at STP?
4. A container has an initial volume of 4.5 L, a pressure of 450 kPa and is at a temperature of 15 oC. If the
container is expanded to 6.5 L while the pressure is decreased to 125 kPa, find the resulting temperature.
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Soda Can Activity
OBJECTIVES
Students will demonstrate the effects of air pressure.
Students will demonstrate that as a gas is heated it expands and as it cools it will contract.
MATERIALS
an empty aluminum soft-drink can
a 1000 mL beaker
a pair of beaker tongs
hot plate
PROCEDURE
1. Fill the large beaker with ice cold water.
2. Put 15 – 20 milliliters of water into the empty soft-drink can.
3. Heat the can on the hot plate at the highest setting. When the water boils, a cloud of condensed vapor will
escape from the opening in the can. Allow the water to boil for about two minutes. Do not let all of the
water evaporate.
4. Using the beaker tongs, grasp the can and quickly invert it and dip it into the water in the pan. Be careful
of the hot water!
5. Record your observation.
6. Clean up your lab station.
OBSERVATION
CONCLUSION
Explain why the can was crushed (discuss the relationships between pressure, volume, and temperature). Why did
you have to heat the can up in order for the can to be crushed?
10
Boyle’s Law and Charles’ Law
The Effect of Changing Size of Container – Boyle’s Law WHAT IF…temperature and moles do not change and we just look at the relationship between pressure and
volume. Our equation would look like this:
P1V1 = P2V2 Boyle’s Law
Boyle’s Law states that at a constant temperature, the volume of a gas is inversely proportional to the pressure
exerted by that gas.
Examples:
a. If a gas is compressed from 2L to 1L, the pressure will
_____________ by a factor of 2.
b. If a gas is expanded from 1L to 3L, the pressures will
_______________ by a factor of 3.
c. Gases cool when they expand and heat when they compress.
Why?
Thus, if you forget to wear your suit in space, you
will_________________!!!
Example Problems
1. The pressure of a 3.5L balloon was determined to be 1.5atm. Assuming that the temperature remained
constant, what would be the volume of the balloon if the pressure was decreased to 0.45atm?
2. At 45oC, a certain container of gas has the volume of 580mL and a pressure of 980mmHg. What would be