GASES Chapter 14. From last chapter… Kinetic Molecular Theory Particles in an ideal gas… –...
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Transcript of GASES Chapter 14. From last chapter… Kinetic Molecular Theory Particles in an ideal gas… –...
GASES
Chapter 14
From last chapter… Kinetic Molecular Theory
• Particles in an ideal gas…– have no ____________.– Have ____________ collisions. – are in ____________, random, straight-line
motion.– Don’t ____________________each other.– have an avg. KE directly related to
__________________________
Real Gases
• Particles in a ____________ gas…– have their own volume– attract each other
• Gas behavior is most ideal…– At _______ pressures– At _________ temperatures– In ___________ atoms/molecules
Properties of Gases
• __________________ – gases are easily compressed because of the space between the particles in a gas
• Gases __________ to take the shape and volume of their container
Factors Affecting Gas Pressure• _____________________– more particles have more
collisions with the container walls and thus create more pressure
• _______________ – if you reduce the volume of the container, the particles are more compressed and exert a greater pressure on the walls of the container
• ______________ – increasing temperature increases the kinetic energy of the particles, which then strike the walls of the container with more energy
Remember?Units of Pressure
• KEY UNITS AT SEA LEVEL
101.325 kPa (kilopascal)
1 atm
760 mm Hg
760 torr
14.7 psi
*These are all equivalent amounts of pressure
Standard Temperature & PressureStandard Temperature & Pressure
____ ______
_____ __________-OR-
STP
The Gas Laws14.2
The Gas Laws14.2
Boyle’s Law• The pressure and volume of a gas
are inversely related – at constant mass & temp
P
V
GIVEN:
V1 = 100. mL
P1 = 150. kPa
V2 = ?
P2 = 200. kPa
WORK:
Gas Law Problem• A gas occupies 100. mL at 150. kPa. Find its
volume at 200. kPa.
BOYLE’S LAW
P V
V
T
Charles’ Law• The volume and absolute
temperature (K) of a gas are directly related – at constant mass & pressure
GIVEN:
V1 = 473 cm3
T1 = 36°C = 309K
V2 = ?
T2 = 94°C = 367K
WORK:
Gas Law Problem• A gas occupies 473 cm3 at 36°C. Find its
volume at 94°C.
CHARLES’ LAW
T V
P
T
Gay-Lussac’s Law• The pressure and absolute
temperature (K) of a gas are directly related – at constant mass & volume
GIVEN:
P1 = 765 torr
T1 = 23°C = 296K
P2 = 560. torr
T2 = ?
WORK:
Gas Law Problem• A gas’ pressure is 765 torr at 23°C. At what
temperature will the pressure be 560. torr?
GAY-LUSSAC’S LAW
P T
Combined Gas Law
GIVEN:
V1 = 7.84 cm3
P1 = 71.8 kPa
T1 = 25°C = 298 K
V2 = ?
P2 = 101.325 kPa
T2 = 273 K
WORK:
Gas Law Problem• A gas occupies 7.84 cm3 at 71.8 kPa & 25°C.
Find its volume at STP.
P T VCOMBINED GAS LAW
V
n
Avogadro’s Law
• The volume and number of moles of a gas are directly related – at constant temperature & pressure
GIVEN:
V1 = 36.7 L
n1 = 1.5 mol
V2 = 16.5 L
n2 = ?
WORK:
Gas Law Problem• Consider two sample of N2 gas. Sample 1 contains 1.5 mol
of N2 and has a volume of 36.7 L at 25°C and 1 atm. Sample 2 has a volume of 16.5 L at 25°C and 1 atm. Calculate the number of moles of N2 in Sample 2.
AVOGADRO’S LAW
n V
14.3 - Ideal Gas Law
UNIVERSAL GAS CONSTANTR=0.0821
Latm/molKR=8.315
dm3kPa/molK
GIVEN:
P = ? atm
n = 0.412 mol
T = 16°C = 289 K
V = 3.25 LR = 0.0821Latm/molK
WORK:
Ideal Gas Law Problem• Calculate the pressure in atmospheres of 0.412
mol of He at 16°C & occupying 3.25 L.
14.4 - Dalton’s Law of Partial Pressures
• The partial pressure of a gas is the pressure that the gas would exert if it were alone in the container.
• Dalton’s Law of Partial Pressures says that the total pressure of a mixture of gas is equal to the sum of the partial pressures of all gases in the mixture. Or,
Note: you can calculate the partial pressures of the gases if they behave ideally using the ideal gas law (P = nRT/V)
Dalton’s Law Example
• A 2.0 L flask contains a mixture of nitrogen gas and oxygen gas at 25°C. The total pressure of the gaseous mixture is 0.91 atm, and the mixture is known to contain 0.050 mol of N2. Calculate the partial pressure of oxygen and the moles of oxygen present.
Graham’s Law of Effusion
• ____________ is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout
• ____________ is when a gas escapes through a tiny hole in its container
• Gases of _______ molar mass diffuse and effuse _________ than gases of _________ molar mass
Graham’s Law of Effusion
• The rate of effusion of a gas is ____________ proportional to the square root of the gas’s molar mass.
• This equation compares effusion rates for two gases
Graham’s Law Problem
• Calculate the ratio of the velocity of hydrogen molecules (H2) to the velocity of carbon dioxide (CO2) molecules at the same temperature.
Gas Stoichiometry
• ______________of a gas is the volume that is occupied by 1 mol of an ideal gas at STP.–1 mol of gas occupies __________
• Yes, we are going back to those 3 step problems…
Gas Stoichiometry Problem
Quicklime, CaO, is produced by heating calcium carbonate. Calculate the volume of carbon dioxide produced at STP from the decomposition of 152 g of calcium carbonate according to the reaction
CaCO3 (s) CaO (s) + CO2 (g)