Warm Up: (5 minutes) GET BINDERS OUT READY TO TAKE NOTES! (-5 FOR ANYONE NOT READY ONCE bell rings!) We have learned about four states of matter, in which of the following 3 states do particles move the MOST  solids, liquids, or gases? (Do not have to write question, but answer in complete sentence). What is the relationship between how fast these particles move and the shape and volume this state of matter has? (2 sentences) (Write question and answer)

Announcements New TOP 10 Doughnuts Friday Morning Quiz on Friday – States of Matter & Gas Laws Grades – next class TEDx Interviews today

Answer to DO NOW What is the relationship between how fast these particles move and the shape and volume this state of matter has? (2 sentences) Particles in a gas are well separated with no regular arrangement/pattern. Gas particles move freely/collide at high speeds.

GASES! Get your notes set up: Title: Gas Laws Date your notes in top right

Kinetic Molecular Theory How particles in matter behave! All matter is composed of particles Particles are in constant motion Particles also collide with other particles and may lose some energy

SOLID Molecular Motion: Atoms vibrate in place Packed closely together DO NOT NEED TO COPY, you already know! Molecular Motion: Atoms vibrate in place Packed closely together Arranged in a geometric pattern Heat Index: At its freezing point Attraction: Very close together

LIQUID Molecular Motion: atoms able to slide by one another DO NOT NEED TO COPY Molecular Motion: atoms able to slide by one another Attraction: Still able to cling to each other More kinetic energy To slip out of the solid state, the particles had to gain in kinetic energy Heat Index: Melting Point – when particles slip from a solid to a liquid

PLASMA Most common state in the universe Positively charged particles DO NOT NEED TO COPY Most common state in the universe Positively charged particles Molecular Motion: Moves extremely fast – electrons are stripped off Electrically charged

GAS Molecular Motion: Freely floats around Attraction: No Attraction Will fill whatever container it is living in. Heat Index: Vaporization – when liquid becomes a gas Must escape its attractive forces

Standards by ClayCo Just finished  SPS5a. Compare and contrast the atomic/molecular motion of solids, liquids, gases and plasmas. Now  SPS5b. Relate temperature, pressure, and volume of gases to the behavior of gases.

Enduring understanding  For gaseous substances, pressure, volume, and temperature are interdependent.

OBJECTIVES YOU will be able to identify Boyle’s Law, Charles Law, & Guy-Lussac’s Law YOU will be able to relate temperature, pressure, and volume to the behavior of gases.

NEW VOCAB Today we are covering: Intermolecular attraction – The amount of "stick togetherness" Temperature – intensity of heat Pressure - exertion of force upon a surface by an object (force per unit of area) Specific Heat - amt of heat per unit mass required to raise the temp by one degree Celsius

Which balloon has HIGHER pressure? Vote: 1 2 Gases- Pressure Which balloon has HIGHER pressure? Vote: 1 2

Gases- Pressure What is it? Pressure is the amount of force exerted on a container from within, it is caused by gas particles colliding with each other. Do MANY or FEW collisions cause a lot of pressure? MANY, the more particles collide the more they Hit the walls of their container, putting force on the walls Does having MORE or FEWER particles cause many collisions? MORE, the more particles there are the more collisions there will be

Boyle’s Law Robert Boyle (1627 – 1691) British Decrease the volume of the container of gas + a constant temperature = pressure of the gas will increase Increase the volume of the container of gas + constant temperature = pressure of gas will decrease

(inversely proportional) Boyle’s Law As the pressure of a gas increases the volume of that gas decreases . When Temperature is constant. (inversely proportional)

Pressure and Volume (WHEN THE AMOUNT OF GAS IS CONSTANT) Use arrow (up = increase, down = decrease) to fill in the blanks under the diagram V V P P

Pressure and Volume (WHEN THE AMOUNT OF GAS IS CONSTANT) Use arrow (up = increase, down = decrease) to fill in the blanks under the diagram V V P P

Boyles Law P1V1=P2V2

Charles Law Jacques Charles (1746 – 1823) – French Volume of gases increases with increasing temperature as long as pressure doesn’t change. Volume of gases decreases with decreased temperature as long as pressure doesn’t change.

(directly proportional) Charles’s Law As the temperature of a gas increases the volume of that gas increases . The pressure is constant. (directly proportional)

Temperature Temperature

Charles Law V1 = V2 T1 T2

(directly proportional) Guy-Lussac’s Law As the temperature of a gas increases the pressure of that gas increases . When volume is constant. (directly proportional)

Temperature Temperature

Guy Lussac’s Law P1 = P2 T1 T2

Practice BOYLE Prediction  solve P1 = 20 atm V1 = 1 L P2 = 10 atm V2 = ? (greater than or less than 1 L?) Atm = atmospheric pressure (units of pressure)

Practice CHARLES Prediction  solve T1 = 300 K V1 = 5 L T2 = 150 K V2 = ? (greater than or less than 5 L)

Practice GUY LUSSAC Prediction  solve P1 = 20 atm T1 = 100 K P2 = 80 atm T2 = ? (greater than or less than 100 K)

Conclusion (2 min) In your notes, write down your answer to this question: What does the set up of each equation tell us about how those two variables affect each other?

Boyle's gas law states: the volume of a gas is inversely proportional to the pressure of the gas when temperature is held constant. Gay-Lussac's law states: @ constant volume, the pressure of a gas is directly proportional to its temperature. Charles' Law states: If the pressure of a gas sample is kept constant, the volume of the sample will vary directly with the temperature