chapter 10 – gas laws. kinetic molecular theory (kmt) particles of matter are always in motion....
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Chapter 10 – Gas Laws
Kinetic Molecular Theory (KMT)
Particles of matter are always in motion.
The KMT describes any property based on the particle motion
Review: Solids = Rotational
Liquids = Rotational & Vibrational
Gases = Rotational, Vibrational & Translational
KMT
Ideal Gas = A gas that acts “perfectly” as expected. Does not really exist, but it is possible to be close to it.
KMT - Assumptions
1. Gases are made of large numbers of tiny particles
2. Particles of a gas are in random, constant straight line motion
3. Collisions of particles are elastic4. There are no attractive or repulsive
forces between particles5. As temperature increases, speed and
energy of the particles increases
http://mc2.cchem.berkeley.edu/Java/molecules/
KMT
KMT
KE = ½ mv2
**Large molecules move slowly; Small molecules move quickly
Properties of Gases
1. Most IDEAL when LOW Pressure and HIGH Temperature
Why???
2. Expansion – Fill entire container
3. Fluidity – Flow due to minimal external bonds
4. Low Density – d = m/v
Properties of Gases
5. Compressibility – Can push particles together to make smaller total volume
6. Diffusion – Mix / Spread out without stirring
Rate1/Rate2 = √Molar Mass2/√M Mass1
Example: How much faster is Hydrogen compared to Oxygen Gas?
Real vs. Ideal Gases
Real Gas = Gas that disobeys an assumption of the KMT of Gases
1. The particles of a real gas have volume themselves. This is ignored by the KMT.
2. Particles of a real gas have attractive and repulsive forces. These are ignored by the KMT.
Qualitative Description of Gases
• Volume of the gas sample
• Pressure – Caused by gas particles hitting the sides of the container
• Temperature of the gas sample
• Number of moles (particles) of the gas
Qualitative Description of Gases
1. Volume vs. Pressure
2. Temperature vs. Volume
3. Temperature vs. Pressure
Qualitative Description of Gases
4. Moles vs. Pressure
5. Moles vs. Volume
Pressure and Temperature Units
mmHg
torr (1 torr = 1 mmHg)
atm (1 atm = 760 mmHg)
kPa (1 atm = 101.325 kPa)
Pressure conversion chart will be given to Academic Classes only
Standard Temperature = 0oCStandard Pressure = 1 atm
STP =
Pressure and Temperature Units
Temperature Conversion Equations will be given to Academic Classes only
K = oC + 273.15
oC = K – 273.15
Pressure and Temperature Units
Practice Problems:
Measuring Pressure
Barometer=A tube filled with Mercury in a “puddle” of mercury.
Measuring Pressure
Barometer
Measuring Pressure
Manometers = Measures Pressure of a Gas Sample
Closed Manometer:
Gas
Closed End – A vacuum
U-Tube with Hg
Pgas = Hg Level Difference
Measuring PressureOpen Manometers:
Pgas = Patm Pgas = Patm + Hg Diff Pgas = Patm – Hg Diff
Equal Levels: Higher on Atm Side: Higher on Gas Side:
Skip P=F/A
10.3 – Quantitative Description of Gases
Gas Laws = Numerical descriptions of gas behaviors
1. Boyle’s Law – Volume and PressureP1V1 = P2V2 (will be given to Academic)Examples:
10.3 – Quantitative Description of Gases
2. Charles’ Law – Temperature and Volume*Temps must be in Kelvin!!
(will be given to Academic)
Examples:
1 2
1 2
V V
T T
10.3 – Quantitative Description of Gases
3. Gay-Lussac’s Law – Pressure and Temperature
*Temps must be in Kelvin!!
(will be given to Academic)
Examples:
1 2
1 2
P P
T T
10.3 – Quantitative Description of Gases
1 1 2 2
1 2
P V P V
T T
1 1 2 2
1 2
P V P V
T T
4. Combined Gas Law – A combination of Boyle’s, Charles’, Gay-Lussac’s
*Temps must be in Kelvin!!
This is really the only one you need to know!
(will be given to Academic)
If Temperature is CONSTANT = = P1V1 = P2V2
If Pressure is CONSTANT = =
1 2
1 2
V V
T T
1 1 2 2
1 2
P V P V
T T
10.3 – Quantitative Description of Gases
4. Combined Gas Law – A combination of Boyle’s, Charles’, Gay-Lussac’s
*Temps must be in Kelvin!!
(will be given to Academic)1 1 2 2
1 2
P V P V
T T
Examples:
More Practice:
10.3 – Quantitative Description of Gases
Dalton’s Law of Partial Pressures
Ptotal = P1 + P2 + P3 + …
(will be given to Academic)
Examples:
Water Displacement (a form of Dalton’s Law)Collecting Gas THROUGH Water
The gas collected contains not only the experimental gas, it also contains WATER VAPOR from the water evaporating!
The container is moved either up or down to make the gas levels EQUAL. This makes the PRESSURE INSIDE = PRESSURE OUTSIDE!
Ptotal = Patm Pgas + PH2O =
Demos
1. Balloon + Flask
2. Galileo’s Thermometer
3. Handboiler
4. Drinking Bird
5. Vacuum Pump Tricks
6. Egg + Flask
7. Soda Can Crushing