1. what is matter? 2. what are the three phases of matter? setup cornell notes titled, “gases”

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1. What is matter? 2. What are the three phases of matter? up cornell notes titled, “Gas

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1. What is matter?

2. What are the three phases of matter?

Setup cornell notes titled, “Gases”

Everything that has mass and takes up space is called matter.

Solid, liquid, gas

44

GASESGASES

Why do gases have different propertiesThan solids and liquids?

Atomic composition (what atoms make up a substance) also affects physical properties.

55

Importance of Gases Importance of Gases

• Airbags fill with NAirbags fill with N22 gas in an gas in an accident. accident.

• Gas is generated by the Gas is generated by the decomposition of sodium decomposition of sodium azide, NaNazide, NaN33..

• 2 NaN2 NaN33 ---> 2 Na + 3 N ---> 2 Na + 3 N22

66

THREE STATES OF THREE STATES OF MATTERMATTER

THREE STATES OF THREE STATES OF MATTERMATTER

77General General Properties of Properties of

GasesGases• There is a lot of “free” There is a lot of “free”

space in a gas.space in a gas.

• Gases can be expanded Gases can be expanded infinitely.infinitely.

• Gases fill containers Gases fill containers uniformly and completely.uniformly and completely.

• Gases diffuse and mix Gases diffuse and mix rapidly.rapidly.

88

Kinetic Molecular Theory

• Kinetic = to move

• Kinetic energy vs. Potential energy

– Kinetic energy: object is moving

– Potential energy: stored energy, is the ability of a system to do work due to its position or internal structure

99

Kinetic Molecular Theory

• Kinetic-molecular theory explains the different properties of solids, liquids, and gases.

• describes the behavior of matter in terms of particles in motion.

1010

Kinetic Molecular Theory• Gases consist of small

particles separated by empty space.

• Gas particles are too far apart to experience significant attractive or repulsive forces.

• Gas particles are in constant random motion and do collide

• An elastic collision is one in which no kinetic energy is lost.

1111

Kinetic Molecular Theory

• Kinetic energy of a particle depends on mass and velocity.

1212Explaining the Behavior of

Gases

Section 12-1

Great amounts of space exist between gas particles.

Compression reduces the empty spaces between particles.

1313

Diffusion vs. Effusion

• Diffusion is the movement of one material through another.

• Effusion is a gas escaping through a tiny opening.

1414

DO NOW – 4/14/10• 1. Draw a picture of 3 different containers

with the particles that compose a gas, liguid, and solid. Which has more empty space?

• 2. Do gas particles…

• Move? Collide? Increase or decrease speed with a temperature increase?

Setup Cornell Notes: “Intro to Gas Laws”

1515

Objectives:

• By the end of the period, you should be able to….

• 1. Describe the movement of gas particles

• 2. Define Pressure, Boyles Law, and Charles Law

• 3. Apply the concepts of pressure, volume, and temperature change to gaseous systems

1616

Agenda

• Do Now

• Notes: “Intro to Gas Laws”

• Activity: outside “Ring of Ping”

• Exit Slip

1717

Intro to Gas Laws

1818Why do our ears sometimes hurt when we are flying on

airplanes?• Airplane ear is the stress exerted on your

eardrum and other middle ear tissues when the air pressure in your middle ear and the air pressure in the environment are out of balance.

• You may experience airplane ear at the beginning of a flight when the airplane is climbing or at the end of a flight when the airplane is descending.

• These fast changes in altitude cause air pressure changes and can trigger airplane ear

1919

2020

What is air Pressure?

Pressure is defined as force per unit area.

• Measured in atmospheres (atm)

• Gas particles exert pressure when they collide with the walls of their container.

• The more they collide with the walls of the container, the higher the pressure

2121

Properties of Properties of GasesGases

Gas properties can be modeled Gas properties can be modeled using math. using math.

• V = volume of the gas (L)V = volume of the gas (L)• T = temperature (K)T = temperature (K)

–ALL temperatures MUST be ALL temperatures MUST be in Kelvin!!! No Exceptions!in Kelvin!!! No Exceptions!

• n = amount (moles)n = amount (moles)• P = pressureP = pressure

(atmospheres) (atmospheres)

2222

PressurPressuree

Pressure of air is Pressure of air is measured with a measured with a BAROMETERBAROMETER (developed by (developed by Torricelli in 1643)Torricelli in 1643)

Hg rises in tube until force of Hg Hg rises in tube until force of Hg (down) balances the force of (down) balances the force of atmosphere (pushing up). atmosphere (pushing up). (Just like a straw in a soft (Just like a straw in a soft drink)drink)

P of Hg pushing down related to P of Hg pushing down related to

• Hg densityHg density

• column heightcolumn height

2323PressurPressureeColumn height measures Column height measures Pressure of atmospherePressure of atmosphere

• 1 standard atmosphere 1 standard atmosphere (atm) *(atm) *

= 760 mm Hg (or torr) *= 760 mm Hg (or torr) *

= 29.92 inches Hg *= 29.92 inches Hg *

= 14.7 pounds/in= 14.7 pounds/in2 2 (psi)(psi) **HD onlyHD only

= 101.3 kPa (SI unit is = 101.3 kPa (SI unit is PASCAL) PASCAL) ** HD onlyHD only

= about 34 feet of water!= about 34 feet of water!

2424

What is Temperature?

• Temperature is a measure of the average kinetic energy (energy of motion) of the particles in a sample of matter.

2525

Gas Laws Simulator

• Record your observations to the right

2626

Activity: “The Ring of Ping”

• Expectations for going outside:–Absolutely NO TALKING in the hallway

» 1 person talks, we ALL go back to the classroom and do an activity from the book

» Once we are outside, No horseplay, everyone is on task or we come back to the classroom

2727

Activity: “The Ring of Ping”

• Ring of Ping–Form a circle: you will represent a container

that has a gas inside of it

–3 volunteers will be my gas particles» You will bounce off of the sides of the container and

bump into one another

» Follow a straight line

» Stay at the same speed

» Be serious and vizualize what you saw in the simulator

2828

Activity: “The Ring of Ping”

• Container people:–When someone bumps into you, you must say

“Ping”

• 1 volunteer will record all of the pings

• Time keeper

2929

Exit Slip

• Explain the relationship you observed in our activity outside between volume, pressure, and temperature

–At least 4 sentences• Turn in last weeks HW: Chap 10 and 11 vocab

with pictures

3030

Start Homework – due Fri

• Read pages 402-410

• Copy down and define the vocabulary on page 402

• Answer questions on page 410

3131

Pressure Conversions

A. What is 475 mm Hg expressed in atm?

1 atm

760 mm Hg

B. The pressure of a tire is measured as 29.4 psi.

What is this pressure in mm Hg?

760 mm Hg

14.7 psi = 1.52 x 103 mm Hg

= 0.625 atm475 mm Hg x

29.4 psi x

3232

Pressure Conversions

A. What is 2 atm expressed in torr?

B. The pressure of a tire is measured as 32.0 psi.

What is this pressure in kPa?

3333Boyle’s Boyle’s LawLawP P αα 1/V 1/VThis means Pressure This means Pressure

and Volume are and Volume are INVERSELY INVERSELY (oppositely) (oppositely) PROPORTIONAL if PROPORTIONAL if moles and moles and temperature are temperature are constant (do not constant (do not change). For change). For example, P goes up example, P goes up as V goes down.as V goes down.

PP11VV11 = P = P22 V V22

Robert Boyle Robert Boyle (1627-1691). (1627-1691). Son of Earl of Son of Earl of Cork, Ireland.Cork, Ireland.

3434

Boyle’s Law and Boyle’s Law and Kinetic Molecular Kinetic Molecular

TheoryTheory

Boyle’s Law and Boyle’s Law and Kinetic Molecular Kinetic Molecular

TheoryTheory

P proportional to 1/VP proportional to 1/V

3535

Boyle’s LawBoyle’s LawBoyle’s LawBoyle’s Law

A bicycle pump is a A bicycle pump is a good example of good example of Boyle’s law. Boyle’s law.

As the volume of the As the volume of the air trapped in the air trapped in the pump is reduced, its pump is reduced, its pressure goes up, pressure goes up, and air is forced into and air is forced into the tire.the tire.

3636

Charles’s Charles’s LawLaw

If n and P are If n and P are constant, constant, then V then V αα T T

V and T are directly V and T are directly proportional.proportional.

VV11 V V22

==

TT11 T T22

• If one temperature goes If one temperature goes

up, the volume goes up!up, the volume goes up!

Jacques Charles (1746-Jacques Charles (1746-1823). Isolated boron and 1823). Isolated boron and studied gases. Balloonist.studied gases. Balloonist.

3737

Charles’s original balloonCharles’s original balloon

Modern long-distance balloonModern long-distance balloon

3838

Charles’s LawCharles’s Law

3939

Gay-Lussac’s LawGay-Lussac’s Law

If n and V are If n and V are constant, constant, then P then P αα T T

P and T are directly P and T are directly proportional.proportional.

PP11 P P22

==

TT11 T T22

• If one temperature goes If one temperature goes

up, the pressure goes up!up, the pressure goes up!

Joseph Louis Gay-Joseph Louis Gay-Lussac (1778-1850)Lussac (1778-1850)

4040Gas Pressure, Gas Pressure, Temperature, and Temperature, and Kinetic Molecular Kinetic Molecular

TheoryTheory

Gas Pressure, Gas Pressure, Temperature, and Temperature, and Kinetic Molecular Kinetic Molecular

TheoryTheory

P proportional to TP proportional to T

4141

Combined Gas Law

• The good news is that you don’t have to remember all three gas laws! Since they are all related to each other, we can combine them into a single equation. BE SURE YOU KNOW THIS EQUATION!

P1 V1 P2 V2

=

T1 T2

No, it’s not related to R2D2

4242

Combined Gas Law

If you should only need one of the other gas laws, you can cover up the item that is constant and you will get that gas law!

= P1 V1

T1

P2 V2

T2

Boyle’s Law

Charles’ Law

Gay-Lussac’s Law

4343

Combined Gas Law Problem

A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29°C. What is the new temperature(°C) of the gas at a volume of 90.0 mL and a pressure of 3.20 atm?

Set up Data Table

P1 = 0.800 atm V1 = 180 mL T1 = 302 K

P2 = 3.20 atm V2= 90 mL T2 = ??

4444

CalculationP1 = 0.800 atm V1 = 180 mL T1 = 302 KP2 = 3.20 atm V2= 90 mL T2 = ??

P1 V1 P2 V2

= P1 V1 T2 = P2 V2 T1

T1 T2

T2 = P2 V2 T1

P1 V1

T2 = 3.20 atm x 90.0 mL x 302 K

0.800 atm x 180.0 mL

T2 = 604 K - 273 = 331 °C

= 604 K

4545

Learning Check

A gas has a volume of 675 mL at 35°C and 0.850 atm pressure. What is the temperature in °C when the gas has a volume of 0.315 L and a pressure of 802 mm Hg?

4646

One More Practice Problem

A balloon has a volume of 785 mL on a fall day when the temperature is 21°C. In the winter, the gas cools to 0°C. What is the new volume of the balloon?

4747And now, we pause for this commercial message from STP

OK, so it’s really not THIS kind of STP…

STP in chemistry stands for Standard Temperature and Pressure

Standard Pressure = 1 atm (or an equivalent)

Standard Temperature = 0 deg C (273 K)

STP allows us to compare amounts of gases between different pressures and temperatures

STP allows us to compare amounts of gases between different pressures and temperatures

4848

Try This One

A sample of neon gas used in a neon sign has a volume of 15 L at STP. What is the volume (L) of the neon gas at 2.0 atm and –25°C?

4949

Avogadro’s Avogadro’s HypothesisHypothesis

Equal volumes of gases at the same Equal volumes of gases at the same T and P have the same number of T and P have the same number of molecules.molecules.

V = n (RT/P) = knV = n (RT/P) = kn

V and n are directly related.V and n are directly related.

twice as many twice as many moleculesmolecules

5050

Avogadro’s Hypothesis Avogadro’s Hypothesis and Kinetic Molecular and Kinetic Molecular

TheoryTheory

Avogadro’s Hypothesis Avogadro’s Hypothesis and Kinetic Molecular and Kinetic Molecular

TheoryTheory

P proportional to nP proportional to n

The gases in this The gases in this experiment are all experiment are all measured at the measured at the same T and V.same T and V.

5151

IDEAL GAS LAWIDEAL GAS LAW

Brings together gas Brings together gas properties.properties.

Can be derived from Can be derived from experiment and theory.experiment and theory.

BE SURE YOU KNOW BE SURE YOU KNOW THIS EQUATION!THIS EQUATION!

P V = n R TP V = n R T

5252

Using PV = nRTUsing PV = nRTP = PressureP = Pressure

V = VolumeV = Volume

T = TemperatureT = Temperature

N = number of molesN = number of moles

R is a constant, called the R is a constant, called the Ideal Gas ConstantIdeal Gas Constant

Instead of learning a different value for R for all the Instead of learning a different value for R for all the possible unit combinations, we can just possible unit combinations, we can just memorizememorize oneone value and value and convert the units to match R.convert the units to match R.

R = 0.0821R = 0.0821L • atm Mol • K

5353

Using PV = nRTUsing PV = nRTHow much NHow much N22 is required to fill a small room is required to fill a small room

with a volume of 960 cubic feet (27,000 L) with a volume of 960 cubic feet (27,000 L) to 745 mm Hg at 25 to 745 mm Hg at 25 ooC?C?

SolutionSolution

1. Get all data into proper units1. Get all data into proper units

V = 27,000 LV = 27,000 L

T = 25 T = 25 ooC + 273 = 298 KC + 273 = 298 K

P = 745 mm Hg (1 atm/760 mm Hg) P = 745 mm Hg (1 atm/760 mm Hg) = 0.98 atm = 0.98 atm

And we always know R, 0.0821 L atm / mol KAnd we always know R, 0.0821 L atm / mol K

5454

Using PV = nRTUsing PV = nRTHow much NHow much N22 is req’d to fill a small room with a volume of 960 is req’d to fill a small room with a volume of 960

cubic feet (27,000 L) to P = 745 mm Hg at 25 cubic feet (27,000 L) to P = 745 mm Hg at 25 ooC?C?

SolutionSolution

2. Now plug in those values and solve for 2. Now plug in those values and solve for the unknown.the unknown.

PV = PV = nnRTRT

n = (0.98 atm)(2.7 x 10 4 L)

(0.0821 L • atm/K • mol)(298 K)n =

(0.98 atm)(2.7 x 10 4 L)

(0.0821 L • atm/K • mol)(298 K)

n = 1.1 x 10n = 1.1 x 1033 mol (or about 30 kg of gas) mol (or about 30 kg of gas)

RT RTRT RT

5555

Learning Check

Dinitrogen monoxide (N2O), laughing gas, is used by dentists as an anesthetic. If 2.86 mol of gas occupies a 20.0 L tank at 23°C, what is the pressure (mm Hg) in the tank in the dentist office?

5656

Learning Check

A 5.0 L cylinder contains oxygen gas at 20.0°C and 735 mm Hg. How many grams of oxygen are in the cylinder?

5757Deviations from Deviations from Ideal Gas LawIdeal Gas Law

• Real molecules have

volume.

The ideal gas consumes the entire amount of available volume. It does not account for the volume of the molecules themselves.

• There are intermolecular forces.

An ideal gas assumes there are no attractions between molecules. Attractions slow down the molecules and reduce the amount of collisions.

– Otherwise a gas could not condense to become a liquid.

5858

Gases in the AirThe % of gases in air Partial pressure (STP)

78.08% N2 593.4 mm Hg

20.95% O2 159.2 mm Hg

0.94% Ar 7.1 mm Hg

0.03% CO2 0.2 mm Hg

PAIR = PN + PO + PAr + PCO = 760 mm Hg 2 2 2

Total Pressure 760 mm Hg

5959Dalton’s Law of Partial Dalton’s Law of Partial PressuresPressures

What is the total pressure in the flask?What is the total pressure in the flask?

PPtotaltotal in gas mixture = P in gas mixture = PAA + P + PBB + ... + ...Therefore, Therefore,

PPtotaltotal = P = PHH22OO + P + POO22 = 0.48 atm = 0.48 atm

Dalton’s Law: total P is sum ofDalton’s Law: total P is sum of PARTIALPARTIAL pressures.pressures.

2 H2 H22OO2 2 (l) ---> 2 H(l) ---> 2 H22O (g) + OO (g) + O2 2 (g)(g)

0.32 atm 0.32 atm 0.16 atm 0.16 atm

6060

Dalton’s Dalton’s LawLaw

John DaltonJohn Dalton1766-18441766-1844

6161Health NoteWhen a scuba diver is several hundred feet under water, the high pressures cause N2 from

the tank air to dissolve in the blood. If the diver rises too fast, the dissolved N2 will form

bubbles in the blood, a dangerous and painful condition called "the bends". Helium, which is inert, less dense, and does not dissolve in the blood, is mixed with O2 in

scuba tanks used for deep descents.

6262Collecting a gas “over water”

• Gases, since they mix with other gases readily, must be collected in an environment where mixing can not occur. The easiest way to do this is under water because water displaces the air. So when a gas is collected “over water”, that means the container is filled with water and the gas is bubbled through the water into the container. Thus, the pressure inside the container is from the gas AND the water vapor. This is where Dalton’s Law of Partial Pressures becomes useful.

6363Table of Vapor Pressures for Water

6464

Solve This!

A student collects some hydrogen gas over water at 20 degrees C and 768 torr. What is the pressure of the H2 gas?

768 torr – 17.5 torr = 750.5 torr

6565

GAS DENSITYGAS DENSITYGAS DENSITYGAS DENSITY

HighHigh densitydensity

Low Low densitydensity

22.4 L of ANY gas AT STP = 1 mole

6666Gases and Gases and StoichiometryStoichiometry

2 H2 H22OO2 2 (l) ---> 2 H(l) ---> 2 H22O (g) + OO (g) + O2 2 (g)(g)

Decompose 1.1 g of HDecompose 1.1 g of H22OO22 in a flask with a in a flask with a volume of 2.50 L. What is the volume of Ovolume of 2.50 L. What is the volume of O22 at STP?at STP?

Bombardier beetle Bombardier beetle uses decomposition of uses decomposition of hydrogen peroxide to hydrogen peroxide to defend itself.defend itself.

6767Gases and Gases and StoichiometryStoichiometry

2 H2 H22OO2 2 (l) ---> 2 H(l) ---> 2 H22O (g) + OO (g) + O2 2 (g)(g)

Decompose 1.1 g of HDecompose 1.1 g of H22OO22 in a flask with a volume of 2.50 L. in a flask with a volume of 2.50 L. What is the volume of OWhat is the volume of O22 at STP? at STP?

SolutionSolution1.1 g1.1 g HH22OO22 1 mol H 1 mol H22OO22 1 mol O 1 mol O22 22.4 L O 22.4 L O22

34 g H34 g H22OO22 2 mol H 2 mol H22OO22 1 mol O 1 mol O22

= 0.36 L O2 at STP

6868

Gas Stoichiometry: Practice!

A. What is the volume at STP of 4.00 g of CH4?

B. How many grams of He are present in 8.0 L of gas at

STP?

6969

What if it’s NOT at STP?

• 1. Do the problem like it was at STP. (V1)

• 2. Convert from STP (V1, P1, T1) to the stated conditions (P2, T2)

7070

Try this one!

How many L of O2 are needed to react 28.0 g NH3

at 24°C and 0.950 atm?

4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)

7171

GAS DIFFUSION AND GAS DIFFUSION AND EFFUSIONEFFUSION

• diffusiondiffusion is the is the gradual mixing of gradual mixing of molecules of molecules of different gases.different gases.

• effusioneffusion is the is the movement of movement of molecules through a molecules through a small hole into an small hole into an empty container.empty container.

HONORS HONORS onlyonly

7272GAS DIFFUSION AND GAS DIFFUSION AND

EFFUSIONEFFUSION

Graham’s law governs Graham’s law governs effusion and diffusion effusion and diffusion of gas molecules.of gas molecules.

Thomas Graham, 1805-1869. Professor Thomas Graham, 1805-1869. Professor in Glasgow and London.in Glasgow and London.

Rate of effusion is Rate of effusion is inversely proportional to inversely proportional to its molar mass.its molar mass.

Rate of effusion is Rate of effusion is inversely proportional to inversely proportional to its molar mass.its molar mass.

M of AM of B

Rate for B

Rate for A

HONORS HONORS onlyonly

7373

GAS DIFFUSION AND GAS DIFFUSION AND EFFUSIONEFFUSION

Molecules effuse thru holes in a Molecules effuse thru holes in a rubber balloon, for example, at a rubber balloon, for example, at a rate (= moles/time) that israte (= moles/time) that is

• proportional to Tproportional to T

• inversely proportional to M.inversely proportional to M.

Therefore, He effuses more rapidly Therefore, He effuses more rapidly than Othan O22 at same T. at same T.

HeHe

HONORS HONORS onlyonly

7474

Gas DiffusionGas Diffusionrelation of mass to rate of relation of mass to rate of

diffusiondiffusion

Gas DiffusionGas Diffusionrelation of mass to rate of relation of mass to rate of

diffusiondiffusion

• HCl and NH3 diffuse from opposite ends of tube.

• Gases meet to form NH4Cl

• HCl heavier than NH3

• Therefore, NH4Cl forms closer to HCl end of tube.

• HCl and NH3 diffuse from opposite ends of tube.

• Gases meet to form NH4Cl

• HCl heavier than NH3

• Therefore, NH4Cl forms closer to HCl end of tube.

HONORS HONORS onlyonly

At 100°C, water becomes water vapor, a gas. Molecules can move randomly over large distances.

Below 0°C, water solidifies to become ice. In the solid state, water molecules are held together in a rigid structure.

Between 0°C and 100 °C, water is a liquid. In the liquid state, water molecules are close together, but can move about freely.

•Have an indefinite shape•Have an indefinite volume

Kinetic Molecular Theory:

Molecules are moving in random patterns with varying amounts of distance between the particles.