1. Part II
Gas Laws and more

2. Bring in a clear plastic 2 liter bottle with cap.
We will be making a Squidy to take home near the end of this set of lessons.

3. New Area of Focus: Gases and Other Laws.
Copyright © 2010 Ryan P. Murphy

4. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water.
Make an observation about the volume of a gas and temperature. Switch them periodically.
Cold
Hot

5. Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature.
Sometimes referred to as Amontons' Law

6. Charles Law: Volume of a gas increases with temperature
Charles Law: Volume of a gas increases with temperature. (Gases expand with heat).
Copyright © 2010 Ryan P. Murphy

8. The formula for the law is:
Volume
________ = K
Temp
Copyright © 2010 Ryan P. Murphy

9. The formula for the law is:
Volume
________ = K
Temp
Copyright © 2010 Ryan P. Murphy

10. The formula for the law is:
Volume
________ = K
Temp
Copyright © 2010 Ryan P. Murphy

11. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water.
Make an observation about the volume of a gas and temperature. Switch them periodically.
Cold
Hot

12. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water.
Make an observation about the volume of a gas and temperature. Switch them periodically.
Cold
Hot

13. Demonstration: Fit a balloon to the top of a bottle and place in pan with hot and cold water.
Make an observation about the volume of a gas and temperature. Switch them periodically. V =K T
Cold
Hot

14. Video / Demonstration. Making a Hero’s Engine. (6 minutes)
Explain at the end

15. V is the volume of the gas.
Copyright © 2010 Ryan P. Murphy

16. V is the volume of the gas.
T is the temperature of the gas (measured in Kelvin)
Copyright © 2010 Ryan P. Murphy

17. V is the volume of the gas.
T is the temperature of the gas (measured in Kelvin)
K is a constant.
Copyright © 2010 Ryan P. Murphy

18. V is the volume of the gas.
T is the temperature of the gas (measured in Kelvin)
K is a constant.
K= The universal constant in the gas equation: pressure times volume = R times temperature; equal to joules per Kelvin per mole.
Copyright © 2010 Ryan P. Murphy

19. V is the volume of the gas.
T is the temperature of the gas (measured in Kelvin)
K is a constant.
K= The universal constant in the gas equation: pressure times volume = R times temperature; equal to joules per Kelvin per mole.
Copyright © 2010 Ryan P. Murphy

20. This law means that when the temperature goes up, the volume of the gas goes up.

21. This law means that when the temperature goes up, the volume of the gas goes up.

22. This law means that when the temperature goes up, the volume of the gas goes up.

23. This law means that when the temperature goes up, the volume of the gas goes up.

24. This law means that when the temperature goes up, the volume of the gas goes up.
As the molecules heat up they move around faster and collide more often.

25. This law means that when the temperature goes up, the volume of the gas goes up.
As the molecules heat up they move around faster and collide more often.
Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature.

26. This law means that when the temperature goes up, the volume of the gas goes up.
As the molecules heat up they move around faster and collide more often.
Gay-Lussac's Law: The pressure exerted on the sides of a container by an ideal gas of fixed volume is proportional to its temperature.

27. This law means that when the temperature goes up, the volume of the gas goes up.

28. This law means that when the temperature goes up, the volume of the gas goes up.

29. This law means that when the temperature goes up, the volume of the gas goes up.

30. This law means that when the temperature goes up, the volume of the gas goes up.

31. This law means that when the temperature goes up, the volume of the gas goes up.

32. This law means that when the temperature goes up, the volume of the gas goes up.

33. This law means that when the temperature goes up, the volume of the gas goes up.

34. This law means that when the temperature goes up, the volume of the gas goes up.

35. This law means that when the temperature goes up, the volume of the gas goes up.
When the temperature goes down, the volume of the gas decreases.

36. You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
Copyright © 2010 Ryan P. Murphy

37. The air molecules are moving very slowly so the ball is flat.
You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
The air molecules are moving very slowly so the ball is flat.
Copyright © 2010 Ryan P. Murphy

38. The air molecules are moving very slowly so the ball is flat.
You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
The air molecules are moving very slowly so the ball is flat.
Cooler, so molecules are slower and colliding less often
Copyright © 2010 Ryan P. Murphy

39. The air molecules are moving very slowly so the ball is flat.
You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
The air molecules are moving very slowly so the ball is flat.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.
Cooler, so molecules are slower and colliding less often
Copyright © 2010 Ryan P. Murphy

40. The air molecules are moving very slowly so the ball is flat.
You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
The air molecules are moving very slowly so the ball is flat.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.
Cooler, so molecules are slower and colliding less often
Copyright © 2010 Ryan P. Murphy

41. The air molecules are moving very slowly so the ball is flat.
You may notice that your sports equipment doesn’t work well when you go out into your garage in the winter.
The air molecules are moving very slowly so the ball is flat.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.
Cooler, so molecules are slower and colliding less often
Copyright © 2010 Ryan P. Murphy

42. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
Copyright © 2010 Ryan P. Murphy

43. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
PSI =
Copyright © 2010 Ryan P. Murphy

44. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
PSI =
Pounds per square inch
Kilopascals : The standard metric unit for measuring air pressure.
Copyright © 2010 Ryan P. Murphy

45. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
PSI =
Pounds per square inch
Kilopascals : The standard metric unit for measuring air pressure.
Copyright © 2010 Ryan P. Murphy

46. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
Copyright © 2010 Ryan P. Murphy

47. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.
Copyright © 2010 Ryan P. Murphy

49. Avogadro’s Law / Hypothesis.
Copyright © 2010 Ryan P. Murphy

50. Avogadro’s Law / Hypothesis
Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.”
Copyright © 2010 Ryan P. Murphy

51. Avogadro’s Law / Hypothesis
Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.”
“I would love to show you my gas laws, will you join me?”
Copyright © 2010 Ryan P. Murphy

52. Avogadro’s Law / Hypothesis
Avogadro’s Law / Hypothesis. “Hello ladies, I am the Italian savant named Amedo Avogadro.”
“I would love to show you my gas laws, will you join me?”
Copyright © 2010 Ryan P. Murphy

53. Avogadro's Law: Equal volumes of gases, at the same temperature and pressure, contain the same number of particles, or molecules.
Copyright © 2010 Ryan P. Murphy

54. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no (or entirely negligible) intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

56. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

57. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

58. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

59. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

60. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

61. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

62. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

63. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

64. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

65. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

66. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

67. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

68. Study a few minutes. Questions will follow.
Gases are made up of molecules which are in constant random motion..
Pressure is due to collisions between the molecules and the walls of the container.
All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic.
(That means that there is no loss of kinetic energy during the collision.)
The temperature of the gas is proportional to the average kinetic energy of the molecules.
There are no intermolecular forces between the gas molecules.
The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.

69. When temperatures get colder, you may need to add some more molecules to get the safe PSI for your vehicle.
Copyright © 2010 Ryan P. Murphy

70. The kinetic movement of molecules causes gas particles to move to open areas.
Copyright © 2010 Ryan P. Murphy

71. The kinetic movement of molecules causes gas particles to move to open areas.
Copyright © 2010 Ryan P. Murphy

72. When pressure is increased on a gas its volume is decreased.

73. When pressure is increased on a gas its volume is decreased.

74. When pressure is increased on a gas its volume is decreased.

75. A B Which container has the higher density?
(Same conditions / same molecules / same temp / in each) A B

76. B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

77. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

78. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

79. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

80. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

81. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

82. A B B Which container has the higher density?
Since density is defined to be the mass divided by the volume, density depends directly on the size of the container in which a fixed mass of gas is confined.

83. Demonstration! Marshmallow Torture
Place Marshmallow into Bell Jar vacuum.
Remove Air from Bell Jar
Record Picture of Marshmallow.
Quickly let air rush back in and observe.

84. Air Pressure Demonstration! Marshmallow Torture
Place Marshmallow into Bell Jar vacuum.
Remove Air from Bell Jar
Record Picture of Marshmallow.
Quickly let air rush back in and observe.
Air Pressure

85. (Marshmallow Expands)
Demonstration! Marshmallow Torture
Place Marshmallow into Bell Jar vacuum.
Remove Air from Bell Jar
Record Picture of Marshmallow.
Quickly let air rush back in and observe.
Air Pressure
No Air Pressure
(Marshmallow Expands)

86. (Marshmallow Expands)
Demonstration! Marshmallow Torture
Place Marshmallow into Bell Jar vacuum.
Remove Air from Bell Jar
Record Picture of Marshmallow.
Quickly let air rush back in and observe.
Air Pressure
No Air Pressure
(Marshmallow Expands)
Vacuum broken

87. Boyle’s Law: Pressure and Volume are inversely proportional.
Copyright © 2010 Ryan P. Murphy

88. Boyle’s Law: Pressure and Volume are inversely proportional.
P is the pressure of the molecules on the container, V is the volume of the container, and k is a constant. The value of k always stays the same so that P and V vary appropriately. For example, if pressure increases, k must remains constant and thus volume will decrease.
Copyright © 2010 Ryan P. Murphy

89. As pressure increases, volume decreases.
As volume decreases, pressure increases.
Copyright © 2010 Ryan P. Murphy

90. As pressure increases, volume decreases.
As volume decreases, pressure increases.
Copyright © 2010 Ryan P. Murphy

91. As pressure increases, volume decreases.
As volume decreases, pressure increases.
Copyright © 2010 Ryan P. Murphy

92. As pressure increases, volume decreases.
As volume decreases, pressure increases.
Copyright © 2010 Ryan P. Murphy

93. “I’m Pressure.” As pressure increases, volume decreases.
As volume decreases, pressure increases.
“I’m Pressure.”
Copyright © 2010 Ryan P. Murphy

94. “I’m Volume.” “I’m Pressure.” As pressure increases, volume decreases.
As volume decreases, pressure increases.
“I’m Volume.”
“I’m Pressure.”
Copyright © 2010 Ryan P. Murphy

96. Very Important! Record in Journal.

102. Gas Laws and more available sheet.

103. Activity! Syringes

104. Activity! Syringes (Safety Goggles Needed)

105. Activity! Syringes
Depress plunger on the syringe.

106. Activity! Syringes Depress plunger on the syringe.
Cover hole with finger.

107. Activity! Syringes Keep thumb on opening.
Depress plunger on the syringe.
Cover hole with finger.
Try and pull handle (gently please).
Why is it difficult?
Keep thumb on opening.

108. Why is it difficult? Activity! Syringes Keep thumb on opening.
Depress plunger on the syringe.
Cover hole with finger.
Try and pull handle (gently please).
Why is it difficult?
Keep thumb on opening.
Why is it difficult?

109. Activity! Syringes Keep thumb on opening.
Answer: It was difficult because your finger created a sealed vacuum and prevented air from entering the chamber.
Keep thumb on opening.

110. Activity! Syringes Keep thumb on opening.
Answer: It was difficult because your finger created a sealed vacuum and prevented air from entering the chamber. Atmospheric pressure is 1 kilogram per square centimeter at sea level.
Keep thumb on opening.

111. Now let’s add some marshmallows into the syringe.
Add a few marshmallows in the syringe,
Push the plunger until it just touches the marshmallows.
Covering the tip of the syringe with your finger, pull the plunger up.
What happened?

112. Now let’s add some marshmallows into the syringe.
Add a few marshmallows in the syringe.
Push the plunger until it just touches the marshmallows.
Covering the tip of the syringe with your finger, pull the plunger up.
Question to Answer… What happened?

113. What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.
When the plunger was pulled out, the pressure decreased so the marshmallow expanded in size.

114. What happened?
When you depressed in the plunger, the air pressure increased.

115. What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.

116. What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.
When the plunger was pulled out, the pressure decreased so the marshmallow expanded in size.

117. Boyles Law What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.
When the plunger was pulled out, the pressure decreased so the marshmallow expanded in size.
Boyles Law

118. Boyles Law What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.
When the plunger was pulled out, the pressure decreased so the marshmallow expanded in size.
Boyles Law

119. Boyles Law What happened?
When you depressed in the plunger, the air pressure increased.
This pushes air bubbles out of the marshmallow and causes it to decrease in size.
When the plunger was pulled out, the pressure decreased so the marshmallow expanded in size.
Boyles Law

120. Gas Laws and more available sheet.

121. Activity! Syringes (Opposite)

122. Activity! Syringes (Opposite)
Fill syringe.

123. Activity! Syringes (Opposite)
Fill syringe.
Cover hole with finger.

124. Activity! Syringes (Opposite)
Fill syringe.
Cover hole with finger.
Try and push handle (gently please).

125. Activity! Syringes (Opposite)
Fill syringe.
Cover hole with finger.
Try and push handle (gently please).
How does this represent Boyles Law?

126. Activity! Syringes (Opposite)
How does this represent Boyles Law?

127. Activity! Syringes (Opposite)
How does this represent Boyles Law?
Answer: As you depress the plunger, you increase pressure and the volume of the gas is decreased.

128. Activity! Syringes (Opposite)
How does this represent Boyles Law?
Answer: As you depress the plunger, you increase pressure and the volume of the gas is decreased.
Please determine how many milliliters you were able to compress the gas inside using the numbers on the syringe.

129. Activity! Syringes (Opposite)
How does this represent Boyles Law?
Answer: As you depress the plunger, you increase pressure and the volume of the gas is decreased.
Please determine how many milliliters you were able to compress the gas inside using the numbers on the syringe.
Answer: You should be able to compress the gas to about 50% of it’s starting volume by hand and then it gets difficult.

132. “Can’t wait to eat my yogurt.”

134. As you inhale, your diaphragm flattens out allowing your chest to expand and allows more air to flow into your lungs.

135. As you inhale, your diaphragm flattens out allowing your chest to expand and allows more air to flow into your lungs.
Air pressure decrease, air then rushes into your lungs.

136. As you exhale, your diaphragm relaxes to a normal state
As you exhale, your diaphragm relaxes to a normal state. Space in chest decreases.

137. As you exhale, your diaphragm relaxes to a normal state
As you exhale, your diaphragm relaxes to a normal state. Space in chest decreases.
Air pressure increases, air then rushes out of your lungs.

138. Which is a inhale, and which is a exhale?B

139. Which is a inhale, and which is a exhale?B

140. Which is a inhale, and which is a exhale?B

141. Which is a inhale, and which is a exhale?B

142. Which is a inhale, and which is a exhale?
Inhale Exhale A B

143. Which is a inhale, and which is a exhale?B A B

144. Which is a inhale, and which is a exhale?B A B

145. Which is a inhale, and which is a exhale?B A B

146. Which is a inhale, and which is a exhale?B A B

147. Which is a inhale, and which is a exhale?
Inhale Exhale A B A B

150. The Bends (Decompression Sickness) – Bubbles form in blood if you rise too quickly because of the rapid decrease in pressure.
Copyright © 2010 Ryan P. Murphy

151. The Bends (Decompression Sickness) – Bubbles form in blood if you rise too quickly because of the rapid decrease in pressure.
A diver must save time to travel to surface slowly so body can adjust.
Copyright © 2010 Ryan P. Murphy

152. Short Area of Focus: Last bit about air pressure (Flight).
Copyright © 2010 Ryan P. Murphy

154. How do planes fly?

155. Early plane (Wright Brothers)

159. Flight: A Simple combination of Bernoulli’s Principle and Newtons 1st Law of Motion.
Copyright © 2010 Ryan P. Murphy

161. An object at rest tends to stay at rest and an object in motion tends to stay in motion with the same speed and in the same direction unless acted upon by an unbalanced force.
Copyright © 2010 Ryan P. Murphy

162. Bernoulli's Principle

163. Bernoulli's Principle
Bernoulli's principle states that for an inviscid flow, an increase in the speed of the fluid occurs simultaneously with a decrease in pressure or a decrease in the fluid's potential energy.

164. Air flows faster over the top of the wing than the bottom making less pressure, higher pressure underneath pushes the wing up.
Copyright © 2010 Ryan P. Murphy

165. Learn more about flight at… http://www.lcse.umn.edu/~bruff/bernoulli.html

167. Propeller uses same principles with air pressure.
Copyright © 2010 Ryan P. Murphy

168. Activity! Teacher will demonstrate ping pong ball levitation with hair dryer.
The airflow from the hair dryer speeds up as it slips by the floating sphere, which creates an area of low pressure around the ball. The high pressure from the dryer surrounds the low around the ball and keeps the ball trapped in midair.

169. Student needed to read explanation
Activity! Teacher will demonstrate ping pong ball levitation with hair dryer.
The airflow from the hair dryer speeds up as it slips by the floating sphere, which creates an area of low pressure around the ball. The high pressure from the dryer surrounds the low around the ball and keeps the ball trapped in midair.
Student needed
to read explanation

170. Activity! Teacher will demonstrate ping pong ball levitation with hair dryer.
The airflow from the hair dryer speeds up as it slips by the floating sphere, which creates an area of low pressure around the ball. The high pressure from the dryer surrounds the low around the ball and keeps the ball trapped in midair.

171. Activity! Teacher will demonstrate ping pong ball levitation with hair dryer.
The airflow from the hair dryer speeds up as it slips by the floating sphere, which creates an area of low pressure around the ball. The high pressure from the dryer surrounds the low around the ball and keeps the ball trapped in midair.

172. Activity! Teacher will demonstrate ping pong ball levitation with hair dryer.
The airflow from the hair dryer speeds up as it slips by the floating sphere, which creates an area of low pressure around the ball. The high pressure from the dryer surrounds the low around the ball and keeps the ball trapped in midair.

173. Activity!
Everyone can try with a bendy straw and ping pong ball.
Or…

174. Activity!
Everyone can try with a bendy straw and ping pong ball.

175. Activity!
Everyone can try with a bendy straw and ping pong ball.

176. Activity! Everyone can try with a bendy straw and ping pong ball.
The stream of air moves at high speed.

177. L Activity! Everyone can try with a bendy straw and ping pong ball.
The stream of air moves at high speed. As should be expected from Bernoulli's equation, this stream of air has a lower pressure than the stationary surrounding air. L

178. Activity!
Everyone can try with a bendy straw and ping pong ball. H
The stream of air moves at high speed. As should be expected from Bernoulli's equation, this stream of air has a lower pressure than the stationary surrounding air. If the ball starts to move to one side of the stream, the high-pressure of the stationary air pushes it back into the stream. L H

179. Box Activity! (Optional)
Light candle directly behind box (non-flammable material) and try and blow out candle.
Box

180. Tube Activity! (Optional)
Light candle directly behind tube / round container of about equal thickness (non-flammable material) and try and blow out candle.
Tube

181. Tube Activity! (Optional)
Light candle directly behind tube / round container of about equal thickness (non-flammable material) and try and blow out candle.
Tube

182. Tube Activity! (Optional)
Light candle directly behind tube / round container of about equal thickness (non-flammable material) and try and blow out candle.
Tube

183. What happened? Why?
The air tended to stick to the curved surface of the bottle. This is called the Coanda effect.

184. Quick Paper Airplane building contest!
Copyright © 2010 Ryan P. Murphy

185. Quick Paper Airplane building contest!
One piece 8 by 11, furthest flight wins, must be a plane with wings.
Copyright © 2010 Ryan P. Murphy

186. Quick Paper Airplane building contest!
One piece 8 by 11, furthest flight wins, must be a plane with wings.
Glider instructions on the next slide for those who need it.
Copyright © 2010 Ryan P. Murphy

187. …

188. Gas Laws and more available sheet.

189. Gas Laws and more available sheet.
Works as a teacher
demonstration.

190. Activity – Pressure and temperature.
Copyright © 2010 Ryan P. Murphy

191. Activity – Pressure and temperature.
Copyright © 2010 Ryan P. Murphy

192. Safety Goggles Required Activity – Pressure and temperature.
Copyright © 2010 Ryan P. Murphy

193. Activity – Pressure and temperature.
Copyright © 2010 Ryan P. Murphy

194. Activity! Temp and Pressure.

195. Activity! Temp and Pressure.
Record temperature inside bottle with cap off under normal atmospheric pressure.

196. Activity! Temp and Pressure.
Record temperature inside bottle with cap off under normal atmospheric pressure.
Pump up bottle using “Fizz Keeper” as much as you can until it doesn’t create more pressure.

197. Activity! Temp and Pressure.
Record temperature inside bottle with cap off under normal atmospheric pressure.
Pump up bottle using “Fizz Keeper” as much as you can until it doesn’t create more pressure.
Record temperature in bottle under pressure.

198. Activity! Temp and Pressure.
Record temperature inside bottle with cap off under normal atmospheric pressure.
Pump up bottle using “Fizz Keeper” as much as you can until it doesn’t create more pressure.
Record temperature in bottle under pressure.
Observe the temperature as you unscrew the cap.

199. Questions for the “Fizz Keeper Activity”
What was the temperature change?
Copyright © 2010 Ryan P. Murphy

200. Questions for the “Fizz Keeper Activity”
What was the temperature change?
How are pressure and temperature related?
Copyright © 2010 Ryan P. Murphy

201. Questions for the “Fizz Keeper Activity”
What was the temperature change?
Copyright © 2010 Ryan P. Murphy

202. Questions for the “Fizz Keeper Activity”
What was the temperature change?
The temperature increased a few degrees with increased pressure.
Copyright © 2010 Ryan P. Murphy

203. Questions for the “Fizz Keeper Activity”
How are pressure and temperature related?
Copyright © 2010 Ryan P. Murphy

204. Questions for the “Fizz Keeper Activity”
How are pressure and temperature related?
They are inversely proportional. When one goes up, the other goes down.
Copyright © 2010 Ryan P. Murphy

205. Very Important! Record in Journal.

206. Copyright © 2010 Ryan P. Murphy

207. As pressure increases, temperature increases.
Copyright © 2010 Ryan P. Murphy

208. As pressure increases, temperature increases.
Copyright © 2010 Ryan P. Murphy

209. As pressure increases, temperature increases.
Copyright © 2010 Ryan P. Murphy

210. As pressure increases, temperature increases.
As pressure decreases, temperature decreases.
Copyright © 2010 Ryan P. Murphy

211. As pressure increases, temperature increases.
As pressure decreases, temperature decreases.
Copyright © 2010 Ryan P. Murphy

212. As pressure increases, temperature increases.
As pressure decreases, temperature decreases.
Copyright © 2010 Ryan P. Murphy

213. Pressure and temperature: Can you explain how this bird will continue to drink thinking about temperature and pressure?
Copyright © 2010 Ryan P. Murphy

215. Answer: Your body heat warms the fluid in the abdomen.
Copyright © 2010 Ryan P. Murphy

216. Answer:
The heat increases the vapor pressure in the abdomen relative to the head (the reverse of what happens when you wet the head).
Copyright © 2010 Ryan P. Murphy

217. Answer:
The fluid rises into the head in response to the pressure difference (moving from high pressure to low pressure).
Copyright © 2010 Ryan P. Murphy

218. Answer: The bird becomes top-heavy, and tips.
Copyright © 2010 Ryan P. Murphy

219. Cool Water wets felt around head Answer:
The bird becomes top-heavy, and tips.
Cool Water
wets felt
around head
Copyright © 2010 Ryan P. Murphy

220. Temperature and Pressure
Copyright © 2010 Ryan P. Murphy

221. Temperature and Pressure
As temp rises, pressure rises
Copyright © 2010 Ryan P. Murphy

222. Temperature and Pressure
As temp rises, pressure rises
As pressure rises, temp rises
Copyright © 2010 Ryan P. Murphy

223. Temperature and Pressure
As temp rises, pressure rises
As pressure rises, temp rises
Copyright © 2010 Ryan P. Murphy

224. Temperature and Pressure
As temp rises, pressure rises
As pressure rises, temp rises
Copyright © 2010 Ryan P. Murphy

225. Temperature and Pressure
As temp rises, pressure rises “Watch out”
As pressure rises, temp rises
Copyright © 2010 Ryan P. Murphy

226. Temperature and Pressure
As temp rises, pressure rises “Watch out”
As pressure rises, temp rises
Copyright © 2010 Ryan P. Murphy

227. Temperature and Pressure
As temp rises, pressure rises “Watch out”
As pressure rises, temp rises “Watch out”
Copyright © 2010 Ryan P. Murphy

228. +

239. +

240. +

242. This photoshop job might look “Funny”.

243. Caution! Graphic Images of burns / the dangers of pressure and temperature.

244. The consequences of severe burns and explosions are not “funny”.
Copyright © 2010 Ryan P. Murphy

248. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

249. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

250. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

251. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

252. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

253. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

254. The ideal gas law: PV = nRT (pressure times volume equals the number of molecules times the gas constant times temperature)
Copyright © 2010 Ryan P. Murphy

255. P= V= n= R= T=
Copyright © 2010 Ryan P. Murphy

256. P=Pressure V=Volume is equal to the.. n= Number of molecules
R= Gas constant = JK m
T= Temperature
Copyright © 2010 Ryan P. Murphy

257. P=Pressure V=Volume is equal to the.. n= Number of molecules
R= Gas constant = JK m
T= Temperature
Mole is a unit of measurement used in chemistry to express amounts of a chemical substance.
Copyright © 2010 Ryan P. Murphy

261. P= V= n= R= T=

262. P= V= n= R= T=

263. P= Pressure V= n= R= T=

264. P= Pressure V= n= R= T=

265. P= Pressure
V= Volume n= R= T=

266. P= Pressure
V= Volume n= R= T=

267. P= Pressure
V= Volume
n= Number of Molecules R= T=

268. P= Pressure
V= Volume
n= Number of Molecules R= T=

269. P= Pressure
V= Volume
n= Number of Molecules
R= Gas Constant T=

270. P= Pressure V= Volume n= Number of Molecules R= Gas Constant T=
8.134 JK m

271. P= Pressure V= Volume n= Number of Molecules R= Gas Constant T=
8.134 JK m

272. P= Pressure V= Volume n= Number of Molecules R= Gas Constant
T= Temperature
8.134 JK m

273. Video Link! (Optional) Khan Academy Ideal Gas Law (Advanced)

274. Activity! Visiting Ideal Gas Law Simulator
How you can use this gas law to find…

275. Activity! Visiting Ideal Gas Law Simulator
How you can use this gas law to find…
Calculating Volume of Ideal Gas: V = (nRT) ÷ P

276. Activity! Visiting Ideal Gas Law Simulator
How you can use this gas law to find…
Calculating Volume of Ideal Gas: V = (nRT) ÷ P
Calculating Pressure of Ideal Gas: P = (nRT) ÷ V

277. Activity! Visiting Ideal Gas Law Simulator
How you can use this gas law to find…
Calculating Volume of Ideal Gas: V = (nRT) ÷ P
Calculating Pressure of Ideal Gas: P = (nRT) ÷ V
Calculating moles of gas: n = (PV) ÷ (RT)

278. Activity! Visiting Ideal Gas Law Simulator
How you can use this gas law to find…
Calculating Volume of Ideal Gas: V = (nRT) ÷ P
Calculating Pressure of Ideal Gas: P = (nRT) ÷ V
Calculating moles of gas: n = (PV) ÷ (RT)
Calculating gas temperature: T = (PV) ÷ (nR)

279. Deflate Gate
Note: Everything is made up for this exercise.

280. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
How did the game balls change through the first half?

281. How did the game balls change through the first half?
Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
How did the game balls change through the first half?
This is going to get confusing for a bit but just stick with it.

282. How did the game balls change through the first half?
Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
How did the game balls change through the first half?
This is going to get confusing for a bit but just stick with it.

283. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
How did the game balls change through the first half?
“Life is easier when using metric”

284. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant?

285. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.

286. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2 ?
Equipment manager

287. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
“Umm that’s part of the controversy”

288. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)

289. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)

290. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi

291. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi

292. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 68ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi
12.5 PSI – 11.8 PSI = 0.7 PSI

293. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 80ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi
12.5 PSI – 11.8 PSI = 0.7 PSI

294. Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 80ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi
12.5 PSI – 11 PSI = 1.5 PSI

295. illegal when in the cold
Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 80ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi
A legal ball turned
illegal when in the cold
12.5 PSI – 11 PSI = 1.5 PSI

296. or was it the ball boy? V? Oh the drama!
Tom Brady inflated his AFC championship footballs to the league minimum of 12.5 PSI or 86, pascals in a locker room that was 80ºF or 20ºC which is K. The outdoor temperature during game time was 51ºF / 10.6ºC or ( K)
Which letters in PV=nrt will change? Which will remain constant? P= pressure and t = temperature will change.
V shouldn’t change as hopefully no air was added or removed. We are then left with p1 / T1 = p2 / T2
It gets a little tricky as we need to add current atmospheric pressure at Gillette Stadium at game time ( Pa)
(86,184.5 Pa Pa) / K = (p Pa) / K
Isolate the lone variable
{[(86,184.5 Pa Pa) / K] * K} Pa = p2
79,800.9 Pa = p2 ---> 11.8 psi
or was it the ball boy? V?
Oh the drama!
12.5 PSI – 11 PSI = 1.5 PSI

297. Activity! Gas Law Simulator.
What happens to molecules when…
Temperature is increased.
Pressure is increased.
Volume is decreased.
Copyright © 2010 Ryan P. Murphy

298. Activity! Gas Law Simulator.
What happens to molecules when…
Temperature is increased.
Pressure is increased.
Volume is decreased.
Copyright © 2010 Ryan P. Murphy

299. Activity! Gas Law Simulator.
What happens to molecules when…
Temperature is increased.
Pressure is increased.
Volume is decreased.
Copyright © 2010 Ryan P. Murphy

300. Activity! Gas Law Simulator.
What happens to molecules when…
Temperature is increased.
Pressure is increased.
Volume is decreased.
Copyright © 2010 Ryan P. Murphy