gas!!! it’s everywhere!!!!. kinetic molecular theory 1.most of the volume occupied by a gas is...
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Gas!!!Gas!!!It’s It’s
Everywhere!!!!Everywhere!!!!
Kinetic Molecular TheoryKinetic Molecular Theory
1. Most of the volume occupied by a gas is empty space
2. Collisions between gas particles are elastic collisions
• Energy is transferred between the particles
Kinetic Molecular Kinetic Molecular TheoryTheory
3. Gas particles are in constant motion
• Possess kinetic energy (energy of motion)
4. Kinetic Energy in a gas depends on the temperature
• KE = ½ mv2
Kinetic Molecular TheoryKinetic Molecular Theory
• Expansion– No definite shape or volume
• Fluidity– Gases flow like liquids
• Low Density– Most of the volume is empty
space
• Compressibility– Since mostly empty space,
particles can be squeezed into a smaller volume
DiffusionDiffusion• Spontaneous mixing of gas particles
caused by their random motion
EffusionEffusion• A process by which gas particles
pass through a small opening
Diffusion vs. EffusionDiffusion vs. Effusion
Real vs. IdealReal vs. Ideal• Ideal Gas – An imaginary gas
that perfectly fits all of the assumptions of the Kinetic Molecular Theory
• Real Gas – A gas that does not behave completely according to the assumptions of the Kinetic Molecular Theory – A real gas can behave like an
ideal gas under high temperature and low pressure conditions
STPSTP
• STP = Standard Temperature and Pressure
Standard Temperature = 0°C Standard Pressure = 1 atm
PressurePressure
• The force per unit area on a surface
• Barometer – a device used to measure atmospheric pressure
Units of PressureUnits of Pressure
• Millimeters of mercury – mmHg• Torr• Atmosphere – atm• Pascal – Pa• Kilopascal - kPa
Important ConversionImportant Conversion
• 1 atm = 760 mmHg• 1 atm = 760 torr• 1 atm = 101.325 kPa
TemperatureTemperature• Kelvin is the standard temperature
scale used when dealing with gases• Absolute zero = 0 K
– Unreachable!
• Temperature in Kelvin = Temperature in Celsius + 273• Temperature in Celsius = Temperature in Kelvin – 273
0°C = 273 K25°C = 298 K (Room Temp)0 K = -273°C (Absolute Zero)
Boyle’s LawBoyle’s Law• The volume of a gas at
constant temperature varies indirectly with pressure.
ExampleExample• The pressure exerted on a 240
mL sample of hydrogen gas at constant temperature is increased from 0.428 atm to 0.724 atm. What will the final volume of the sample be?
• V1 = 240.0 mL
• V2= ?
• P1 = 0.428 atm
• P2 = 0.724 atm
P1V1 = P2V2
(0.428 atm)(240.0 mL) = (0.724 atm)V2
V2 = 142 mL
Charles’ LawCharles’ Law• The volume of a gas at
constant pressure varies directly with the temperature
ExampleExample• A sample of air has a volume
of 140.0 mL at 67°C. At what temperature will its volume be 50.0 mL at constant pressure?
• V1 = 140.0 mL
• V2= 50.0 mL
• T1 = 67°C + 273 = 340 K
• T2 = ?
V1 V2
T1 T2
=V1
V2 T1T2 = =(50.0 mL)(340K)
140.0 mL= 121 K
Gay-Lussac’s LawGay-Lussac’s Law• The pressure of a gas at
constant volume varies directly with the temperature
Combined Gas LawCombined Gas Law
ExampleExample
• A helium filled balloon has a volume of 50.0 L at 25°C and 1.08 atm. What volume will it have at 0.855 atm and 10°C?
SolutionSolution
• V1 = 50.0 L
• V2= ????
• P1 = 1.08 atm
• P2 = 0.855 atm
• T1 = 25°C + 273 = 298 K
• T2 = 10°C + 273 = 283 K
Step 1: List what you are given.
Must Convert to Kelvin!!!!
SolutionSolutionStep 2: Solve the Combined Gas
Law for your unknown.
SolutionSolution
Step 3: Solve!
V2 =(1.08 atm)(50.0 L)(283 K)
(0.855 atm)(298 K)
60.0 L HeV2 =
Dalton’s LawDalton’s Law• The total pressure of a
mixture of gases is equal to the sum of the partial pressures of the component gases.
PT = P1 + P2 + ..... + Pn
ExampleExample• What is the total pressure of
a gas containing a mixture of three gases whose partial pressures are 20 kPa, 10 kPa, and 30 kPa?
PT = P1 + P2 + ..... + Pn
PT = 20 kPa + 10 kPa + 30 kPa
PT = 60 kPa
Ideal Gas LawIdeal Gas Law• The mathematical relationship
among pressure, volume, temperature, and the number of moles of a gas.
ExampleExample• Calculate the volume, in liters,
occupied by 2.00 mol of H2 at 300 K and 1.25 atm. (R = 0.0821)
PV = nRT
V =nRT
P
V =(2.00mol)(0.0821)(300K)
1.25 atm
V = 39.4 L
Avogadro’s LawAvogadro’s Law• Equal volumes of gases at
the same temperature and pressure contain equal numbers of molecules.
Gas StoichiometryGas Stoichiometry
2CO + O2 2CO2
How many liters of oxygen are required to produce 2 L of carbon dioxide?
2L CO2
2L CO2
1L O2= 1L O2