gases. elements that exist as gases at 25 0 c and 1 atmosphere
TRANSCRIPT
Gases
Elements that exist as gases at 250C and 1 atmosphere
• Gases assume the volume and shape of their containers.
• Gases are the most compressible state of matter.
• Gases will mix evenly and completely when confined to the same container.
• Gases have much lower densities than liquids and solids.
Physical Characteristics of Gases
Kinetic Theory of Gases
• KMT Based on 5 Assumptions:
1. G. have large number of particles that are very far apart from each other
relative to their size.
2. Collisions between g. particles and between g. particles and container walls
are elastic. (No net loss of kinetic energy)
Kinetic Theory of Gases cont.
3. G. particles are in constant motion
4. There are no forces of attraction between G. particles.
5. The temperature of a gas depends on the average kinetic energy of the particles of the gas. KE= ½ (mv2). All gases have the same
KE at the same temperature.
Ideal vs. Real Gases
• Ideal gas: hypothetical gas that perfectly fits all of the assumptions of the KMT.
• Real gas: one that does not behave exactly according to the assumptions of the KMT.
• Real gas behavior more likely at high pressures and low temperatures.
Questions
1. What happens to gas particles when a gas is compressed?
2. What happens to gas particles when a gas is heated?
3. Describe the conditions under which a real gas is most likely to behave ideally.
Gases and Pressure
• Pressure: Force per unit area.
Pressure =
Units of Pressure
1 pascal (Pa) = 1 N/m2
1 atm = 760 mmHg = 760 torr
1 atm = 101,325 Pa
4/16/2012
Get out your notebooks and your books if you
have them.
Gases
Gases and Pressure
• Calculate the pressure of the following:
1. F=500N, A= 325cm2
2. F=500N, A= 13cm2
3. F=500N, A= 6.5cm2
Gases
Gases and Pressure• Convert the following
pressures:
1. P = 0.830atm to mmHg, and kPa
2. P = 1.75atm to mmHg and kPa
3. The critical pressure of carbon dioxide is 72.7atm, what is this value in Pa?
Gases
Gases and Pressure• Standard Temperature
and Pressure (STP)
• = 1atm and 0°C
Gases
Dalton’s Law of Partial Pressures• The pressure of each gas in a
mixture is the partial pressure of that gas.
• Dalton’s Law of partial pressures = the total pressure of a gas mixture is the sum of all the partial pressures of the
component gases.
• PT = P1 + P2 + P3 + ….
Gases
Dalton’s Law of Partial Pressures
• Water Displacement, gas collected over water.
• Always mixed with water vapor, which has specific
water pressure.
• Patm = Pgas + PH2O
Gases
Dalton’s Law of Partial Pressures• Three of the primary
components of air are CO2, O2, and N2. In the sample
containing a mixture of only these gases at exactly 1atm, the
partial pressures of PCO2 = 0.285 torr and PN2 = 593.525
torr. What is the partial pressure of oxygen?
Gases
Dalton’s Law of Partial Pressures• Oxygen gas from
decomposition of KClO3, was collected by water
displacement. The barometric pressure and temperature was 731.0 torr and 20.0°C. What
was the partial pressure of the oxygen collected?
4/19/2012
Get out your notebooks
Boyle’s Law
• Volume of a fixed mass of gas varies inversely with pressure at a constant temperature.
• PV = k , k is a constant
• Product always remains the same, so can be written:
• P1V1 = P2V2
Boyle’s Law
Constant temperatureConstant amount of gas
A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?
P1 x V1 = P2 x V2
P1 = 726 mmHg
V1 = 946 mL
P2 = ?
V2 = 154 mL
P2 = P1 x V1
V2
726 mmHg x 946 mL154 mL
= = 4460 mmHg
Charle’s Law• Volume of a fixed mass of gas at
constant pressure varies directly with the Kelvin Temperature.
• V = kT , k is a constant or
Charle’s Law• Kelvin Scale: -273.15ºC, or 0 K. Absolute
Zero at which all movement stops.
• K = 273.15 + ºC
• Convert 50ºC to K
• K = 273.15 +50
• K = 223.15K
Charle’s Law
A sample of carbon monoxide gas occupies 3.20 L at 125 0C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant?
V1 = 3.20 L
T1 = 398.15 K
V2 = 1.54 L
T2 = ?
T2 = V2 x T1
V1
1.54 L x 398.15 K3.20 L= = 192 K
V1/T1 = V2/T2
Guy-Lussac’s Law• Pressure of a fixed mass of
gas at a constant temperature varies directly with the Kelvin Temperature.
• P = kT , k is a constant or
The gas in a container is at a pressure of 3.00atm at 25ºC. Directions on the container warn the user not to keep it in a place where the temp. exceeds 52ºC. What would the pressure in the container be at that temp?
P1 = 3.00 atm
T1 = 298.15 K
P2 = ?
T2 = 325.15K
P2 = T2 x P1
T1
325.15 K x 3.00atm298.15 K= = 3.27atm
P1/T1 = P2/T2
Combined Gas Law• Expression of the relationship between
pressure, volume and temperature of a fixed amount of gas.
Combined Gas LawA helium filled balloon has a volume of 50.0L at 25ºC and 1.08atm. What volume will it have at 0.855atm and 10.0ºC.
P1 = 1.08 atm
T1 = 298.15 KP2 = 0.855atm
T2 = 283.15 K
V2 = T2 x P1 x V1
P2 x T1
283.15 K x 1.08atm x 50.0L298.15 K x 0.855atm
=
= 60.0L
V1 = 50.0 L V2 = ?
Avogadro’s Law
V number of moles (n)
V = k x nConstant temperatureConstant pressure
Ammonia burns in oxygen to form nitric oxide (NO) and water vapor. How many volumes of NO are obtained from one volume of ammonia at the same temperature and pressure?
4NH3 + 5O2 4NO + 6H2O
1 mole NH3 1 mole NO
At constant T and P
1 volume NH3 1 volume NO
Avogadro’s Law
Standard Molar Volume: Volume occupied by 1 mole at STP = 22.4L
1mol gas = 22.4L gas
What Volume does 0.0685mol of gas occupy at STP?
Multiply the amount in moles by the conversion factor, 1mol gas = 22.4L gas
What quantity of gas, in moles, is contained in 2.21L at STP?
Multiply the volume in liters by the conversion factor, 1mol gas = 22.4L gas
Ideal Gas Equation
Charles’ law: V T(at constant n and P)
Avogadro’s law: V n(at constant P and T)
Boyle’s law: V (at constant n and T)1P
V nT
P
V = constant x = RnT
P
nT
PR is the gas constant
PV = nRT
The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).
PV = nRT
R = PVnT
=(1 atm)(22.414L)
(1 mol)(273.15 K)
R = 0.082057 L • atm / (mol • K)
Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.
What is the volume (in liters) occupied by 49.8 g of HCl at STP?
PV = nRT
V = nRTP
T = 0 0C = 273.15 K
P = 1 atm
n = 49.8 g x 1 mol HCl36.45 g HCl
= 1.37 mol
V =1 atm
1.37 mol x 0.0821 x 273.15 KL•atmmol•K
V = 30.6 L
Argon is an inert gas used in lightbulbs to retard the vaporization of the filament. A certain lightbulb containing argon at 1.20 atm and 18 0C is heated to 85 0C at constant volume. What is the final pressure of argon in the lightbulb (in atm)?
PV = nRT n, V and R are constant
nRV
= PT
= constant
P1
T1
P2
T2
=
P1 = 1.20 atm
T1 = 291 K
P2 = ?
T2 = 358 K
P2 = P1 x T2
T1
= 1.20 atm x 358 K291 K
= 1.48 atm
Gas Stoichiometry
What is the volume of CO2 produced at 370 C and 1.00 atm when 5.60 g of glucose are used up in the reaction:
C6H12O6 (s) + 6O2 (g) 6CO2 (g) + 6H2O (l)
g C6H12O6 mol C6H12O6 mol CO2 V CO2
5.60 g C6H12O6
1 mol C6H12O6
180 g C6H12O6
x6 mol CO2
1 mol C6H12O6
x = 0.187 mol CO2
V = nRT
P
0.187 mol x 0.0821 x 310.15 KL•atmmol•K
1.00 atm= = 4.76 L
A sample of natural gas contains 8.24 moles of CH4, 0.421 moles of C2H6, and 0.116 moles of C3H8. If the total pressure of the gases is 1.37 atm, what is the partial pressure of propane (C3H8)?
Pi = Xi PT
Xpropane = 0.116
8.24 + 0.421 + 0.116
PT = 1.37 atm
= 0.0132
Ppropane = 0.0132 x 1.37 atm = 0.0181 atm
Gas diffusion is the gradual mixing of molecules of one gas with molecules of another by virtue of their kinetic properties.
NH3
17 g/molHCl
36 g/mol
NH4Cl
Gas effusion is the process by which gas particles pass through a tiny opening.