Honors Chem Chapters 10, 11, and 12. Kinetic Molecular Theory (KMT) Molecules are constantly in...
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Transcript of Honors Chem Chapters 10, 11, and 12. Kinetic Molecular Theory (KMT) Molecules are constantly in...
Honors ChemChapters 10, 11, and 12
Kinetic Molecular Theory (KMT)Molecules are constantly in motion and
collide with one another and the wall of a containerParticles move faster with increased
temperatureGases are made of mostly empty space and just
a few fast moving particles.
Properties of GasesLow DensityExpansionCompressibility FluidityDiffusion/Effusion
Nature of GasesDiffusion: spontaneous mixing of gases
Nature of GasesEffusion: gas particles
spontaneously pass through a small opening
Graham’s Law of Diffusion (or Effusion)
Smaller, lighter gas molecules move faster through the air than larger, heavier gas molecules.
“Lighter, faster, farther”
Graham’s Law of Diffusion (or Effusion)
Graham’s Law: Rewrittenr = rate MM= Molar Mass d = distance t = time light = lighter gas heavy = heavy gas
Kinetic Molecular Theory (KMT)Molecules are constantly in motion and
collide with one another and the wall of a containerParticles move faster with increased
temperatureGases are made of mostly empty space and just
a few fast moving particles.
Ideal GasIdeal Gas: a gas that perfectly conforms to
assumed gas behavior (doesn’t exist)
Most gases are described using real conditions and variables
Variables of Gases(P) Pressure
(V) Volume
(T) Temperature
(n) Amount of gas in moles
PressureMeasures: Force exerted by moving gas particle collisions with their container
Pressure UnitsUnits: 1 atm (atmosphere) of pressure is the
average pressure at sea level
Important Conversions: 1 atm = 760 mmHg (millimeters of Mercury)
= 760 torr= 101.3 kPa (kilo Pascals)= 14.7 psi (pounds per square
inch)
VolumeMeasures: amount of space that a gas
occupies
Units: Liters (L)
Important Conversions: 1 L = 1000mL
TemperatureMeasures: average kinetic energy of gas
particles.
Units: Kelvin (K)The Celsius scale is NOT used for gases
because gases can still have kinetic energy at negative and 0o C.
Kelvin Scale and Absolute ZeroAbsolute Zero = 0 Kelvin represents the
temperature at which a gas has NO kinetic energy
Converting TemperatureImportant Conversions:
oC + 273 = K
K – 273 = oC
STPSTP = Standard Temperature and Pressure
Exactly 0oC and 1 atm
At STP, one mole of gas (6.02 x1023 particles)occupies 22.4 L If a gas is not held at STP, then volume is
recalculated
Gas VariablesA variable is a factor that is liable to change.
Pressure, temperature, and volume of a gas are liable to change.
Pressure, volume, and temperature are interdependent. When variable changes, they all do.
The Combined Gas Law Relates pressure, temperature, volume, and
moles of a gas Relates initial and final conditionsVariables that do not change are constants
and not included in the equation
The Combined Gas Law Equation
The left side (1) represents the initial conditions of the gas
The right side (2) represents the final conditions of the gas
Charles’ Law: Volume and Temp
What changes? And How?Volume increases, temperature increases
What stays the same? Pressure and moles are held constant (toss ‘em)
Charles’ Law: Equation
Remember: Temperatures must be in Kelvin
2
2
1
1
T
V
T
V
Charles’ Law: GraphDirect Relationship: both variables increase
together
Charles Law: Simulation
Charles’ Law: Video Demo
Charles’ Law : ExampleA gas sample at 25 oC and 752 mL is heated
to 50 oC, what is the new volume?
Boyle’s Law : Pressure and Volume
What changes? And How? When Pressure increases, Volume decreases
What stays the same? Temperature and moles are held constant (toss
‘em)
Boyle’s Law : Equation
Remember: Pressure units on both sides of the equation must be the same
P1V1 = P2V2
Boyle’s Law: GraphInverse Relationship: an increase in one
variable with a simultaneous decrease in the other
Boyle’s Law: Simulation
Boyle’s Law: Video Clip
Boyle’s Law ExampleQ: A 1.0 L sample of gas is held at standard
pressure, 1.0 atm. The pressure of the gas is reset to 152 mmHg. What is the new volume of the gas?
Gay-Lussac’s Law: Pressure and Temperature
What changes? And how? As temperature of a gas increases, the pressure
also increasesWhat stays the same?
Volume and moles are held constant (toss ‘em)
Gay-Lussac’s Law: Equation
Pressure units on both sides of the equation must be the same
Temperature must be in Kelvin
2
2
1
1
T
P
T
P
Gay-Lussac’s Law: GraphDirect Relationship: Both variables increase
together
Gay-Lussac’s Law: Simulation
Gay-Lussac’s Law: Video Clip
Gay-Lussac’s Law: Example
Q: A gas has a pressure of 0.370 atm at 50.0 °C. What is the pressure at standard temperature?