GASES
bullPressurebull Temperaturebullnumber of moleculesbullVolume
Parameters to describe gases
force = m x a = kg x ms2 = Newton area (N)Barometer ndash a device used to measure
atmospheric pressureEvangelista Torricelli (early 1600s) used mercury for the first type of barometer
PRESSURE
The SI unit for pressure is named after Blaise Pascal
A Pascal is defined as 1 Newtonacting on an area of one square meter 1 Nm2
Units of pressure760 mm Hg = 760 torr = 1 atmosphere (atm) =
1013 kPa (kilopascals) = 147 psi
Relationship between Pressure Force and AreaForce = mass x acceleration
(On Earth acceleration is a constant due to gravity)
Force =
500 N
Force =
500 N
Area of contact = 325 cm2
Pressure = force area
= 500 N = 15 Ncm2
325 cm2
Area of contact = 13 cm2
Pressure = force area
= 500 N = 385 Ncm2
13cm2
Area of contact = 65 cm2
Pressure = force area
= 500 N = 77 Ncm2
65 cm2
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
bullPressurebull Temperaturebullnumber of moleculesbullVolume
Parameters to describe gases
force = m x a = kg x ms2 = Newton area (N)Barometer ndash a device used to measure
atmospheric pressureEvangelista Torricelli (early 1600s) used mercury for the first type of barometer
PRESSURE
The SI unit for pressure is named after Blaise Pascal
A Pascal is defined as 1 Newtonacting on an area of one square meter 1 Nm2
Units of pressure760 mm Hg = 760 torr = 1 atmosphere (atm) =
1013 kPa (kilopascals) = 147 psi
Relationship between Pressure Force and AreaForce = mass x acceleration
(On Earth acceleration is a constant due to gravity)
Force =
500 N
Force =
500 N
Area of contact = 325 cm2
Pressure = force area
= 500 N = 15 Ncm2
325 cm2
Area of contact = 13 cm2
Pressure = force area
= 500 N = 385 Ncm2
13cm2
Area of contact = 65 cm2
Pressure = force area
= 500 N = 77 Ncm2
65 cm2
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
force = m x a = kg x ms2 = Newton area (N)Barometer ndash a device used to measure
atmospheric pressureEvangelista Torricelli (early 1600s) used mercury for the first type of barometer
PRESSURE
The SI unit for pressure is named after Blaise Pascal
A Pascal is defined as 1 Newtonacting on an area of one square meter 1 Nm2
Units of pressure760 mm Hg = 760 torr = 1 atmosphere (atm) =
1013 kPa (kilopascals) = 147 psi
Relationship between Pressure Force and AreaForce = mass x acceleration
(On Earth acceleration is a constant due to gravity)
Force =
500 N
Force =
500 N
Area of contact = 325 cm2
Pressure = force area
= 500 N = 15 Ncm2
325 cm2
Area of contact = 13 cm2
Pressure = force area
= 500 N = 385 Ncm2
13cm2
Area of contact = 65 cm2
Pressure = force area
= 500 N = 77 Ncm2
65 cm2
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
The SI unit for pressure is named after Blaise Pascal
A Pascal is defined as 1 Newtonacting on an area of one square meter 1 Nm2
Units of pressure760 mm Hg = 760 torr = 1 atmosphere (atm) =
1013 kPa (kilopascals) = 147 psi
Relationship between Pressure Force and AreaForce = mass x acceleration
(On Earth acceleration is a constant due to gravity)
Force =
500 N
Force =
500 N
Area of contact = 325 cm2
Pressure = force area
= 500 N = 15 Ncm2
325 cm2
Area of contact = 13 cm2
Pressure = force area
= 500 N = 385 Ncm2
13cm2
Area of contact = 65 cm2
Pressure = force area
= 500 N = 77 Ncm2
65 cm2
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Relationship between Pressure Force and AreaForce = mass x acceleration
(On Earth acceleration is a constant due to gravity)
Force =
500 N
Force =
500 N
Area of contact = 325 cm2
Pressure = force area
= 500 N = 15 Ncm2
325 cm2
Area of contact = 13 cm2
Pressure = force area
= 500 N = 385 Ncm2
13cm2
Area of contact = 65 cm2
Pressure = force area
= 500 N = 77 Ncm2
65 cm2
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Standard temperature and pressure are definedas 1 atm of pressure and 0C
When describing gases Kelvin temperature is typically used
Kelvin = degC + 273
STP
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Grahamrsquos Law
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
NH3 + HCl NH4Cl
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Grahamrsquos law of Effusion
The rates of effusion ofgases at the same T andP are inversely proportional to thesquare roots of their molar masses
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Derivation of Grahamrsquos LawComparing two gases ldquoArdquo and ldquoBrdquoAt the same T their KE is equal
KEA = KEB
frac12 MAvA2 = frac12 MBvB
2
Multiplying both sides by 2 and rearranging tocompare velocities gives
vA2 = MB
vB2 MA
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Now take the square root of both sides
=
This shows that =
This can also be used when dealing with densitiesof gases
= =
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
The total pressure of a mixture of gases isequal to the sum of the partial pressures ofthe component gases
PT = P1 + P2 + P3 +
Daltonrsquos Law of partial pressures
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
bull Many gases are collected over water thus according to Daltonrsquos law of partial pressures you must account for the vapor pressure of the water
Patm = Pgas + PH2O
A table of water vapor pressures will be provided for you
COLLECTING GASES OVER WATER
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Boylersquos Law - 1662pressure-volume relationship thevolume of a fixed mass of gas variesinversely with the pressure at constanttemperature
PV = kP1V1 = P2V2
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Boylersquos Law graph
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
volume-temperature relationship volume of a fixed massof gas at constant pressure varies directly with the Kelvintemperature) His experiments showed that all gases expand to thesame extent when heated through the same temperatureinterval Charles found that the volume changes by 1273of the original volume for each Celsius degree at constantpressure and an initial temperature of 0C
V = k V1 = V2
T T1 T2 (Kelvin temp)
Charlesrsquos Law - 1787
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Charlesrsquos Law graph
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
pressure-temperature relationship The pressure of a fixed mass of gas at constant volume variesdirectly with the Kelvin temperature For everyKelvin of temperature change the pressure of aconfined gas changes by 1273 of the pressure at0C
P = k P1 = P2 (Kelvin temp)
T T1 T2
Gay-Lussacrsquos Law - 1802
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Gay-Lussac graph
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Combined gas law
pressure volume and temperature relationship
PV = k P1V1 = P2V2
T T1 T2
(Kelvin temp)
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
at a constant T and P the volumes of gaseousreactants and products can be expressed asratios of small whole numbers
Gay-Lussacrsquos Law of Combining Volumes - 1808
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Avogadrorsquos Law
equal volumes of gases at the same T and Pcontain the same number of molecules The volume occupied by one mole of a gas atSTP is known as
standard molar volume of gas 224 liters
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
bull The Ideal Gas Law is the mathematical relationship among pressure volume temperature and the number of moles of a gas
bull Combining Boylersquos Law Charlesrsquos Law and Avogadrorsquos Law gives us V = nRT or more
P
commonly seen as PV = nRT
Ideal Gas Law
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
R = PV = (1 atm)(224 l) = 0082 latm nT (1 mol)(27315K) molK
Other values for R (depending on P units)624 ltorr (or mm Hg) 8314 l kPa mol K mol K
R ndash the ideal gas law constant
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Variations on the ideal gas law can be used to findMolar mass or density (n [moles] = mM)
PV = mRT or M = mRT m= mass M PV M = molar mass
Density is mV so substituting that into the ideal gas equation gives us
M = mRT = DRT which then gives us D = MP PV P RT
Variations on the ideal gas law
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Deviations of real gases from ideal behavior
bull The molecules of an ideal gas are assumed to occupy no space and have no attractions for each other Real molecules however do have finite volumes and they do attract one another
bull In 1873 Johannes van der Waals accounted for this behavior by devising a new equation (based on the ideal gas law) to describe these deviations
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
P = nRT - n2a V-nb V2
Correction for Correction for volume of molecules molecular attractions
The volume is decreased by the factor nb which accounts for thefinite volume occupied by gas molecules The pressure is decreased by the second term which accounts for the attractiveforces between gas molecules The magnitude of a reflects howstrongly the gas molecules attract each other The more polar the molecules of a gas are the more they will attract each other
At very high pressures and very low temperatures deviationsfrom ideal behavior may be considerable
Van der Waals equation
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Good videos for Gases
bull Leidenfrost Effect of H2Ohttpwwwwimpcomwateruphill bull bull httpwwwyoutubecomwatchv=gojuu3AJajAbull ldquoboiling water at room temperaturerdquobull bull httpwwwyoutubecomwatchv=nmKIZtg9itAbull Balloons and marshmallowsbull bull Grahamrsquos Law
httpwwwyoutubecomwatchv=Ff1eL_8kQLAbull
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-
Additional videos
bull Avogadros Law Avogadros Law (1447 min)Boyles Law Boyles Law (541 min)
bull Charles Law Charles Law (641 min)bull Combined Gas Law Combined Gas Law (648 min)bull Ideal Gas Law Ideal Gas Law Introduction (618 min) bull How to rearrange the ideal gas law to form any of the
other laws Be Lazy Dont Memorize the Gas Laws (710 min)
bull Where the ideal gas law constant R comes from Ideal Gas Law Where did R come from (331 min)
- Slide 1
- Slide 3
- Slide 4
- Slide 5
- Relationship between Pressure Force and Area
- Slide 7
- Slide 8
- NH3 + HCl NH4Cl
- Grahamrsquos law of Effusion
- Derivation of Grahamrsquos Law
- Slide 12
- Slide 13
- Slide 14
- Boylersquos Law - 1662
- Slide 16
- Slide 17
- Slide 18
- Slide 19
- Slide 20
- Combined gas law
- Slide 22
- Avogadrorsquos Law
- Slide 24
- Slide 25
- Slide 26
- Deviations of real gases from ideal behavior
- Slide 28
- Good videos for Gases
- Additional videos
-