characteristic of gases. the nature of gases gases expand to fill their containers gases are fluid...

Characteristic of

Gases

The Nature of Gases

bull Gases expand to fill their containersbull Gases are fluid ndash they flowbull Gases have low densityndash 11000 the density of the equivalent liquid

or solid

bull Gases are compressiblebull Gases effuse and diffuse

Gases Are Fluids

bull Gases are considered fluids

bull The word fluid means ldquoany substance that can flowrdquo

bull Gas particles can flow because they are relatively far apart and therefore are able to move past each other easily

Gases Have Low Densitybull Gases have much lower densities than

liquids and solids do - WHY ndash Because of the relatively large distances

between gas particles most of the volume occupied by a gas is empty space

bull The low density of gases also means that gas particles travel relatively long distances before colliding with each other

Gases are Highly Compressible

bull Suppose you completely fill a syringe with liquid and try to push the plunger in when the opening is plugged ndash You cannot make the space the liquid takes up become

smaller bull The space occupied by the gas particles is very

small compared with the total volume of the gasbull Applying a small pressure will move the gas

particles closer together and will decrease the volume

Gases Completely Fill a Container

bull A solid has a certain shape and volume

bull A liquid has a certain volume but takes the shape of the lower part of its container

bull In contrast a gas completely fills its container

bull Gas particles are constantly moving at high speeds and are far apart enough that they do not attract each other as much as particles of solids and liquids do

bull Therefore a gas expands to fill the entire volume available

Gas Pressure

Gas Pressurebull Earthrsquos atmosphere commonly known as air is a

mixture of gases mainly nitrogen and oxygen

bull As gas molecules are pulled toward the surface of Earth they collide with each other and with the surface of Earth more often Collisions of gas molecules are what cause air pressure

Measuring Pressure

Pressure = Area

Force Newton (N)

m2 cm2

Units of Pressure

1 atm = 760 torr = 1013 kPa = 760 mmHg

Standard Temperature Pressure (STP)

1 atm 0degC 224 L 1 mole

100 atm 760 mmHg = 760 x 10^2 mmHg

1 Covert 100 atm to mmHg

1 atm

300atm 1013 kPa = 304 kPa

2 Covert 300 atm to kPa

1 atm

3 What is 1000 KPa in atm

1000 kPa

1013 kPa = 09872 atm

1 atm

bull Measures atmospheric pressure

bull The atmosphere exerts pressure on the surface of mercury in the dish

bull This pressure goes through the fluid and up the column of mercury

bull The mercury settles at a point where the pressure exerted downward by its weight equals the pressure exerted by the atmosphere

Measuring Pressure Using Barometer

Gas Theory

Kinetic Molecular Theorybull Particles of matter are ALWAYS in motionbull Volume of individual particles is zerobull Collisions of particles with container walls cause

pressure exerted by gasbull Particles exert no forces on each otherbull Average kinetic energy is proportional to Kelvin

temperature of a gas

bull Ideal gas- imaginary perfect bull gas fitting the theory

Checking for understandingList 5 characteristics of gases12345

List 5 characteristics of gases according to the KMT12345

Gas Laws

Measurable Properties of GasesGases are described by their measurable

properties

bull P = pressure exerted by the gas

bull V = total volume occupied by the gas

bull T = temperature of the gas

bull n = number of moles of the gas

atm

Units

L

K

mol

Gas Laws ndash ABCGG LAWS

bull Abull Bbull Cbull G

bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos

n is proportional to V constant T

P is inversely proportional to V constant T

V is proportional to T constant P P is proportional to T constant V

rahamrsquos Rate of effusion is inversely proportional to square root of gasrsquos molar mass

Pressure-Volume Relationship

Boylersquos Lawbull Pressure and Volume are inversely

proportional at constant temperaturebull Pressure = Volume bull Volume = Pressure

PV = k

P1V 1= P2V2

For ALL calculations

1 Circle the numbers underline what you are looking for

2 Make a list of number you circled using variables

3 Write down the formula4 Derive the formula to isolate the

variable you are looking for5 Plug in the numbers6 Answer according to significant figures

Boylersquos Law CalculationA given sample of gas occupies 523mL at 100 atm The pressure is increased to 197 atm while the temperature stays the same What is the new volume of the gas

P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL

1 A sample of oxygen gas has a volume of 1500mL at a pressure of 0947 atm What will the volume of the gas be at a pressure of 100 atm if the temperature remains constant

P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL

2 If 25 L of a gas at 1100 kPa is expanded to 40 L at constant temperature what will be the new value of pressure

P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa

Temeperature-Volume Relationship Charlersquos

Lawbull Volume and temperature are

proportional at constant pressurebull volume = temperature (K)bull Volume = temperature (K)

= kVT

V1

T1

=V2

T2

KE of the gases volume temperature

Charless Law Calculation A balloon is inflated to 665 mL volume at 27degC It is immersed in a dry-ice bath at minus785degC What is its volume assuming the pressure remains constantV1= 665 mL V2= mLT1= 27degC + 273 K

= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL

1 Helium gas in a balloon occupies 25 L at 3000K The balloon is dipped into liquid nitrogen that is at a temperature of 800K What will be volume of the helium in the balloon at the lower temperature be

V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2

2 A helium filled balloon has a volume of 275 L at 200 degC The volume of the balloon changes to 246 L when placed outside on a cold day What is the temperature outside in degC

V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1

Temperature-Pressure Relationships Gay-Lussacrsquos

Lawbull Pressure and temperature are

proportional at constant volumebull pressure = temperature (K)bull pressure = temperature (K)

= kPT

P1

T1

=P2

T2

Gay-Lussacrsquos Law Calculation

1 An aerosol can containing gas at 101 kPa and 22degC is heated to 55degC Calculate the pressure in the heated can

P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2

2 A sample of helium gas is at 122 kPa and 22degC Assuming constant volume What will the temperature be when the pressure is 203 kPa

P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1

Volume-Molar Relationships Avogadrorsquos

Lawbull Volume and number of moles (n) are

proportional at constant temperature and pressure

bull volume = number of molesbull volume = number of molesbull 224 L for 1 mole of a gas STP

= kVn

V1

n1

=V2

n2

Avogadrorsquos Lawbull What volume of CO2 contains the same

number of molecules as 200mL of O2 at the same conditions

20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP

Checking for understandingState the law

Explain the law in your own words

Write the formula(s)

Boylersquos Law

Charlersquos Law

Gay-Lussacrsquos LawAvogadrorsquos Law

Gas Behavior ndash DiffusionEffusion

bull Diffusion is the movement of particles from regions of higher density to regions of lower density

bull The passage of gas particles through a small opening is called effusion

Effusion

Grahamrsquos Lawbull The molecular speeds vA and vB of gases A

and B can be compared according to Grahamrsquos law of diffusion shown below

bull Grahamrsquos law of diffusion states that the rate of diffusion of a gas is inversely proportional to the square root of the gasrsquos molar massbull Particles of low molar mass travel faster

than heavier particles

A

B

B

A

M

M

r

r

Grahamrsquos Law Calculationbull At the same temperature which

molecule travels faster O2 or H2

2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398

Hydrogen travels 398 times faster than oxygen

Grahamrsquos Law CalculationOxygen molecules have a rate of about 480 ms at

room temperature At the same temperature what is the rate of molecules of sulfur hexafluoride SF6

32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms

Daltonrsquos Lawbull The pressure of each gas in a mixture is

called the partial pressurebull The total pressure of a mixture of gases is

the sum of the partial pressures of the gases This principle is known as Daltonrsquos law of partial pressure

bull Ptotal = PA + PB + PC

Daltonrsquos Law Calculationbull What is the total pressure in a

balloon filled with air (O2 amp N2) if the pressure of the oxygen is 170 mm Hg and the pressure of nitrogen is 620 mm Hg

bullPtotal = POxygen + Pnitrogen

bullPtotal = PA + PB + PChellip

= 170 mmHg + 620 mmHg

= 790 mmHg

Checking for understanding

State the law



Grahamrsquos LawDaltonrsquos Law

Ideal Gas

Molecular Composition of Gases

bull No gas perfectly obeys all four of these laws under all conditions

bull These assumptions work well for most gases and most conditions

bull One way to model a gasrsquos behavior is to assume that the gas is an ideal gas that perfectly follows these laws

bull An ideal gas unlike a real gas bull does not condense to a liquid at low

temperatures bull does not have forces of attraction or

repulsion between the particles and is bull composed of particles that have no volume

Ideal Gas Law

PV = nRTbull P = pressure in atmbull V = volume in litersbull n = molesbull R = proportionality constant

ndash= 00821 L atm molmiddotKbull T = temperature in Kelvins

The combined gas law expresses the relationship between pressure volume and temperature of a fixed amount of gas

Ideal Gas Law CalculationHow many moles of gas are contained

in 224 L liter at 100 atm and 283K

P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles

Calculate the pressure exerted by 43 mol of nitrogen in a 65L of cylinder at 50degC

P = atm V = 65 L

n = 43 mol R = 00821 Latmmol K

T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm

What will be the volume of 111 mol of nitrogen where the temperature is -57degC and pressure is 250 atm

P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =

(111 mol)(00821 Latmmol K) ( 216 K)(250 atm)

= =79 L

Checking for understanding 1 Explain how is ideal gas different from a

normal gas 2 Write the formula for ideal gas3 What variables can be determined by using the formula

Characteristic of Gases

The Nature of Gases

Gases Are Fluids

Gases Have Low Density



Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory

Kinetic Molecular Theory


Gas Laws

Slide 16


Pressure-Volume Relationship Boylersquos Law


Boylersquos Law Calculation

Slide 21

Slide 22

Temeperature-Volume Relationship Charlersquos Law

Charless Law Calculation

Slide 25

Slide 26

Temperature-Pressure Relationships Gay-Lussacrsquos Law


Slide 29

Volume-Molar Relationships Avogadrorsquos Law

Avogadrorsquos Law

Gas Laws (2)

Checking for understanding (2)


Slide 35

Grahamrsquos Law

Grahamrsquos Law Calculation

Grahamrsquos Law Calculation (2)

Daltonrsquos Law

Daltonrsquos Law Calculation


Ideal Gas


Ideal Gas Law

Ideal Gas Law Calculation

Slide 46

Slide 47


The Nature of Gases

bull Gases expand to fill their containersbull Gases are fluid ndash they flowbull Gases have low densityndash 11000 the density of the equivalent liquid

or solid

bull Gases are compressiblebull Gases effuse and diffuse

Gases Are Fluids



















Gas Pressure




Measuring Pressure

Pressure = Area

Force Newton (N)

m2 cm2

Units of Pressure

1 atm = 760 torr = 1013 kPa = 760 mmHg



100 atm 760 mmHg = 760 x 10^2 mmHg


1 atm

300atm 1013 kPa = 304 kPa


1 atm


1000 kPa

1013 kPa = 09872 atm

1 atm






Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47


Gases Are Fluids



















Gas Pressure




Measuring Pressure

Pressure = Area

Force Newton (N)

m2 cm2

Units of Pressure

1 atm = 760 torr = 1013 kPa = 760 mmHg



100 atm 760 mmHg = 760 x 10^2 mmHg


1 atm

300atm 1013 kPa = 304 kPa


1 atm


1000 kPa

1013 kPa = 09872 atm

1 atm






Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47

















Gas Pressure




Measuring Pressure

Pressure = Area

Force Newton (N)

m2 cm2

Units of Pressure

1 atm = 760 torr = 1013 kPa = 760 mmHg



100 atm 760 mmHg = 760 x 10^2 mmHg


1 atm

300atm 1013 kPa = 304 kPa


1 atm


1000 kPa

1013 kPa = 09872 atm

1 atm






Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





Measuring Pressure

Pressure = Area

Force Newton (N)

m2 cm2

Units of Pressure

1 atm = 760 torr = 1013 kPa = 760 mmHg



100 atm 760 mmHg = 760 x 10^2 mmHg


1 atm

300atm 1013 kPa = 304 kPa


1 atm


1000 kPa

1013 kPa = 09872 atm

1 atm






Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47


100 atm 760 mmHg = 760 x 10^2 mmHg


1 atm

300atm 1013 kPa = 304 kPa


1 atm


1000 kPa

1013 kPa = 09872 atm

1 atm






Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47







Gas Theory







Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47








Gas Laws


properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



properties





atm

Units

L

K

mol



bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




bull G

vogadrorsquos

oylesrsquos

harlesrsquos

ay- Lussacrsquos








PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





PV = k

P1V 1= P2V2







P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47








P1V 1= P2V2

P1= 100 atm P2= 197 atm

V1= 523 mL V2= mL

V2=

P1V1

P2

= (100 atm) (523 mL)

(197 atm)

= 265 mL


P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



P1V 1= P2V2

P1= 0947 atm P2= 100 atmV1= 1500 mL V2= mL

V2=

P1V1

P2

=(0947atm) (1500 mL)

(100atm)

= 142mL


P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



P1V 1= P2V2

P1=1100 kPa P2= kPa

V1= 25 L V2= 40 L

P2=

P1V1

V2

=(1100 kPa) ( 25 L)

(40 L)

= 69 kPa




= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





= kVT

V1

T1

=V2

T2



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



= 300 K

T2= -785degC + 273 K

= 1945 KV1

T1

= V2

T2

V1

T1

=V2T2 =(665 mL)( 1945 K)

(300 K)

= 43 x 10^2 mL


V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



V1= 25 L

T1= 300 K T2= 800 K

V1

T1

= V2

T2

V1

T1

=V2 =(25 L)( 800 K)

(300 K)

= 067 L

V2= mL

T2


V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



V1= 275 L

T1= 20 degC + 273 K = 293

K T2= degC

V1

T1

= V2

T2

V1

V2=T2 =(246 L)( 293 K )

(275 L)

= 26210 K = -1089 degC = -109 degC

V2= 246 L

T1




= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





= kPT

P1

T1

=P2

T2



P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




P1= 101 kPa

T1= 22 degC + 273 K = 295 K T2= 55 degC + 273K = 328 K

P1

T1

=P2

T2

T1

P1=P2 =(101 kPa)( 328 K )

(295 K)

=11 x 10^2 kPa

P2= kPa

T2


P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



P1= 122 kPa

T1= 22 degC + 273 K = 295 K T2= K

P1

T1

=P2

T2

P1

P2=T2 =(203 kPa)(295K)

(122 kPa)

=49 x 10^2 K or 22 x10^2 degC

P2= 203 kPa

T1





= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47






= kVn

V1

n1

=V2

n2



20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




20 mL

Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47


Gas Laws

Combined Gas Law 2

22

1

11

T

VP

T

VP




Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





Boylersquos Law

Charlersquos Law





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





Effusion





A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47






A

B

B

A

M

M

r

r



2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




2

2

2

2

H

O

O

H

M

M

r

r

2

2

H

O

g 202

g 3200 = 398




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




32g

146

r

480ms

6S

g

F

rO2 = 480 ms

rSF6= ms

MO2 = 32g

MSF6= 146g2

6

6

2

O

S

S

O

M

M

r

r F

F

= 220 ms









= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47










= 170 mmHg + 620 mmHg

= 790 mmHg


State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



State the law




Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47


Ideal Gas








Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47









Ideal Gas Law






P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47




P = 100 atm

V = 224 L

n = Moles

R = 00821 Latmmol K

T = 283 K

PV = nRT

RTPV

n =

(00821 Latmmol K) ( 283 K)

(100 atm)(224L) = =964 moles


P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



P = atm V = 65 L


T = 5degC + 273K = 278 K

PV = nRTnRTV

P =

(43 mol)(00821 Latmmol K) ( 278 K)(65 L)

= =15 atm


P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47



P = 250 atm V = L


T = -57degC + 273K = 216 K

PV = nRTnRTP

V =


= =79 L




The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47





The Nature of Gases

Gases Are Fluids




Gas Pressure

Gas Pressure (2)

Measuring Pressure

Slide 10

Slide 11

Gas Theory



Gas Laws

Slide 16





Slide 21

Slide 22



Slide 25

Slide 26



Slide 29


Avogadrorsquos Law

Gas Laws (2)



Slide 35

Grahamrsquos Law



Daltonrsquos Law



Ideal Gas


Ideal Gas Law


Slide 46

Slide 47


characteristic of gases. the nature of gases gases expand to fill their containers gases are fluid...

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