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Gases
Edward Wen, PhD
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Properties of Gases
• expand to completely fill their container• take the shape of their container• low density
much less than solid or liquid state• compressible when pressure is changed.• mixtures of gases are always homogeneous
(common air)• fluid
3
Properties of Gas: Indefinite Shape & Volume
Gas molecules: have enough kinetic energy
and little attractionskeep moving around and
spreading out fill the container of whatever
shape
4
Comparison: Gas, Liquid, SolidState Shape Volume Compress Flow Solid Fixed Fixed No No
Liquid Indef. Fixed No Yes Gas Indef. Indef. Yes Yes
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Kinetic Molecular Theory
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Pressure: Gases PushingWhat are Gas molecules doing?• constantly in motion• as they move and strike a surface,
they push on that surfacepush = force
• Pressure of gas: total amount of force exerted by gas molecules hitting the entire surface at any one instant
pressure = force per unit area
7
Measuring Air Pressure• use a barometer:
column of mercury supported by air pressure
• Force of the air on the surface of the mercury
Gravity on the column of mercury
gravity
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Common Units of PressureUnit Average Air Pressure at
Sea Levelpascal (Pa) 101,325
kilopascal (kPa) 101.325
atmosphere (atm) 1 (exactly)
millimeters of mercury (mmHg) 760 (exactly)
torr (torr) 760 (exactly)
pounds per square inch (psi, lbs./in2) 14.7
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Practice: Convert Pressure between units
• 735.0 mmHg = ? atm
• 35. psi = ? torr
Ans: 0.9671 atm
Ans: 1.8 × 103 torr
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Pressure of a Gas, P• Cause: constant movement of the
gas molecules and their collisions with the surfaces around them
• Pressure depends on:number of gas particles in a given volumevolume of the containeraverage speed of the gas particles
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The Effect of Gas Pressure• whenever there is a Pressure
difference, a gas will flow from area of High pressure area of Low pressure
the bigger the difference in pressure, the stronger the flow of the gas
• if there is something in the gas’ path, the gas will try to push it along as the gas flows
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Gas Pressure in Soda StrawsStraw at idle:Pressure of theair inside the straw = Pressureof the air outsidethe straw liquid levels isthe same on bothsides
Suction of the straw:Pressure of the
air inside the straw is< Pressure
of the air outsidethe straw
liquid is pushedup the straw bythe outside air
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Atmospheric Pressure & Altitude
• Altitude↑ Atmospheric pressure↓• At the surface, P = 14.7 psi, • At 10,000 ft altitude, P = 10.0 psi• Rapid changes in atmospheric pressure may
cause your ears to “pop” an imbalance in pressure on either side of your ear drum (driving or flying)
Demo: Can you make a piece of paper uphold a bottle of water?
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Boyle’s LawFor the gas contained• Pressure of a gas is inversely
proportional to its volume: P 1/V
constant T and amount of gas
• P x V = constant• P1 x V1 = P2 x V2Q: How does the size of an air
bubble change along the way it rises from the deep water to the surface?
∝
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Soda bottle Submarine
Pressure surge when bottle being squeezedVolume of the air inside the dropper decreasesWater filling up the dropperIncreased density of dropper (Massdropper/Volume↑)Dropper sinking!
Pinside
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Boyle’s Experiment• added Hg to a J-
tube with air trapped inside
• Plotting Volume of air vs. Air pressure
Inverse Volume vs Pressure of Air, Boyle's Expt.
0
20
40
60
80
100
120
140
0 0.01 0.02 0.03 0.04 0.05 0.06 0.07 0.08 0.09
Inv. Volume, in-3
Pres
sure
, inH
g
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When you double the pressure on a gas,the volume reduces to one half, (as long as the temperature and amount of gas do not change)
Example:Boyle’s Law
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Example:• A cylinder equipped with a
moveable piston has an applied pressure of 4.0 atm and a volume of 6.0 L. What is the volume if the applied pressure is decreased to 1.0 atm?
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InformationGiven: P1 = 4.0 atm V1 = 6.0 L
P2 = 1.0 atmFind: V2 = ? L
Example:A cylinder equipped with a moveable piston has an applied pressure of 4.0 atm and a volume of 6.0 L. What is the volume if the applied pressure is decreased to 1.0 atm?
Answer: 24 L
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We’re losing altitude.Quick Professor, give yourlecture on Charles’ Law!
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Charles’ LawFor the gas contained and at constant
Pressure:• Volume is directly proportional to
temperature V Tconstant P and amount of gasgraph of V vs T is straight line
• as T increases, V also increases• Kelvin K = °C + 273• V = constant x T
if T measured in Kelvin
2
2
1
1TV
TV
=∝
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Charles’ Law in ActionThe density of common air depends on the
temperature. Higher T, lower Density
• Why the air vents for the air conditioning system are located at the ceiling?
• When measuring the weight of an object, why the high temperature of the object can affect the measurement?
Example:Charles’ Law
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Example:• A sample of gas has a
volume of 2.80 L at an unknown temperature. When the sample is submerged in ice water at 0°C, its volume decreases to 2.57 L. What was the initial temperature in kelvin and in celsius? (assume constant pressure)
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InformationGiven: V1 = 2.80 L
V2 = 2.57 L T2 = 0°CFind: temp1 in K and °C
Example:A gas has a volume of 2.80 L at an unknown temperature. When the sample is at 0°C, its volume decreases to 2.57 L. What was the initial temperature in kelvin and in celsius?
T1 = 297 K = 24 °C
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Gay-Lussac’s LawFor the gas contained at constant
Volume:• Pressure is directly proportional to
temperature P Tconstant V and amount of gasgraph of P vs T is straight line
• as T increases, P also increases• Kelvin K = °C + 273• P = constant x T
if T measured in Kelvin
1 2
1 2
P PT T
=∝
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Gay-Lussac’s Law in Action
The pressure of gas in a sealed container depends on the temperature. Higher T, higher Pressure
• Keep the propane container in a cool place, avoid from direct sunlight.
Example:Gay-Lussac’s Law
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Example:• The tire on a bicycle stored in a cool garage at 18°C
had a pressure of 30. psi. What is the pressure inside the tire after riding the bike at 35°C? Assume the volume of the tire remains constant.
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InformationGiven: T1 = 18°C, P1 = 30. psi
T2 = 35°CFind: P2 in psi.
The tire on a bicycle stored in a cool garage at 18°C had a pressure of 30. psi. What is the pressure inside the tire after riding the bike at 35°C? Assume the volume of the tire remains constant.
T1 = 291 K, T2 = 308 K, P2 = 32 psi
P, V, T
Keep P
P
Keep V
PT V TPV
Keep T
V T
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Avogadro’s Law
• Volume directly proportional to the number of gas molecules
V = constant x nconstant P and Tmore gas molecules = larger volume
• count number of gas molecules by moles
• Equal Volumes of gases contain Equal numbers of molecules
the gas doesn’t matter
2
2
1
1
nV
nV
=
35
Avogadro’s Law
Example:Avogadro’s Law
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Example:• A 4.8 L sample of helium gas contains 0.22 mol helium.
How many additional moles of helium must be added to obtain a volume of 6.4 L? (assume constant pressure and temperature)
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InformationGiven: V1 = 4.8 L, n1 =0.22 mol
V2 = 6.4 LFind: n2, mol and added mol
Example:A 4.8 L sample of helium gas contains 0.22 mol helium. How many additional moles of helium must be added to obtain a volume of 6.4 L?
0.07 mole
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Combined Gas Law• Boyle’s Law : Pressure and
Volumeat constant temperature
• Charles’ Law : Volume and absolute Temperature
at constant pressure
Volume of a sample of gas when both the Pressure and Temperature change
( ) ( )( )
( ) ( )( )2
22
1
11T
VPT
VP •=
•
2
2
1
1TV
TV
=
2211 VPVP •=•
Example:The Combined Gas Law
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InformationGiven: V1 = 158 mL, P1 = 755 mmHg,
t1 = 34°CV2 = 108 mL, t2 = 85°C
Find: P2, mmHg
Example:A sample of gas has a volume of 158 mL at a pressure of 755 mmHg and a temperature of 34°C. The gas is compressed to a volume of 108 mL and heated to 85°C, what is the final pressure in mmHg?
P2 = 31.25 10 mmHg×
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Ideal Gas Law• Combined Gas Law + Avgadro’s Law
Ideal Gas Law
• R is called the Gas Constant• the value of R depends on the units of P and V
R = 0.0821 atm/K · mol convert P to atm and V to L
• Application of Ideal Gas law: when T, P, V of a gas all changes
( ) ( )( ) ( ) nRTPVor R
TnVP
==••
Example:
The Ideal Gas LawRequiring Unit Conversion
44
Example:• Calculate the number of moles of gas in a basketball
inflated to a total pressure of 24.2 psi with a volume of 3.2 L at 25°C
45
InformationGiven: V = 3.2 L, P = 24.2 psi,
t = 25°CFind: n, mol
Example:Calculate the number of moles of gas in a basketball inflated to a total pressure of 24.2 psi with a volume of 3.2 L at 25°C
n 0.22 mol=
46
Air: Mixtures of Gases• Air is a mixture (N2 , O2)• Each gas in the mixture behaves independently
of the other gasesthough all gases in the mixture have the same volume and temperature
all gases completely occupy the container, so all gases in the mixture have the volume of the container
Gas % in Air, by volume Gas % in Air,
by volumenitrogen, N2 78 argon, Ar 0.9oxygen, O2 21 carbon dioxide, CO2 0.03
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Dalton’s Law: Partial Pressure
48
Zn metal reactswith HCl(aq) toproduce H2(g).
Because waterevaporates, somewater vapor getsmixed in withthe H2.
The gas flowsthrough the tubeand bubbles intothe jar, where itdisplaces the water in the jar.
Collecting gas over water
Pgas = PH2O + PH2
49
Standard Conditions (STP)
• Common reference points for comparing
Standard Temperature & Pressure• Standard Pressure = 1.00 atm• Standard Temperature = 0°C = 273 K
50
Molar Volume of a Gas at STPDefinition: The volume of 1 (exact) mole gas at STP • Use the Ideal Gas Law: PV = nRT
L4.22atm1.00
273K Kmole
atmL 0.0821 mole 1
PT R n V =
ו
•×
=××
=
• 1 mole of any gas at STP will occupy 22.4 L==> Molar volume• can be used as a conversion factor
as long as you work at STP1 mol ≡ 22.4 L
51
Molar VolumeSo muchempty spacebetween moleculesin the gas state,
the volume of thegas is not effectedby the size of themolecules, (underideal conditions).
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Density of Gas at STP
• Since every exactly one mole of any gas has a volume of 22.4 L, whereas the mass of such gas would be as the molar mass in grams
• Density of Gas = Molar mass / Molar Volume
Example: • Density of Oxygen gas at STP
= 32.00 g/mol / 22.4 L/mol = 1.43 g/L
53
Density of Common Gases
At STP, the density of common gases (in g/L) as:
• H2 0.0900 • He 0.179• CH4 0.716• N2 1.25 • Air 1.29• O2 1.43• CO2 1.96• Cl2 3.17
• Which one, hydrogen gas or helium gas, is better in blimps in providing lift?
• Why carbon dioxide is used in putting out fire? What if its density is less than the air?
54
Real Gases• Ideal gas laws assume
1) No Attractions between gas molecules2) No Volume: gas molecules do not take up
spacebased on the Kinetic-Molecular Theory
• Real gases: often do not behave like Ideal gases at High pressure (“Squeezed”) or Low temperature (“Frozen”)
55
Ideal vs. Real