The Gas Laws - iss.k12.nc.us
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Transcript The Gas Laws - iss.k12.nc.us
Chapter 14
Chemistry
Remember gases behave
differently
Gases are affected by
Temperature
Pressure
Volume
Boyle’s Law
Robert Boyle
Relationship between pressure and volume
P1V1 = P2V2
Inverse relationship – As volume decreases, pressure
increases
Example Problem
A sample of helium gas in a balloon
is compressed from 4.0 L to 2.5 L at a
constant temperature. If the
pressure of the gas in the 4.0 L
volume is 210 kPa, what will the
pressure be at 2.5 L?
P1V1 = P2V2
Boyle’s Law Activity
Marshmallow in Syringe
Dalton’s Law of Partial Pressures
Charles’s Law
Jacques Charles
Relationship between temperature and pressure
Direct Relationship
V1 = V2
T1
T2
Sample Problem
A gas sample at 40.0oC occupies a volume of 2.32 L. If
the temperature is raised to 75oC, what will the
volume be, assuming the pressure remains constant?
Charles’s Law Activity
Cold Balloon
Bottle Crush
Popcorn
Gay-Lussac’s Law
Relationship between temperature and pressure
Volume must be held constant
Direct relationship
P1 = P2
T1
T2
Sample Problem
The pressure of a gas in a tank is 3.2 atm at 22.o oC. If
the temperature rises to 60 oC, what will be the gas
pressure in the tank?
Combined Gas Law
P1V1 = P2V2
T1
T2
Sample Problem
A gas at 110 kPa and 30.o oC fills a flexible container
with an initial volume of 2.oL . If the temperature is
raised to 80oC and the pressure increased to 440 kPa,
what is the new volume?
Avagadro’s Principle
Equal volumes of gases at the same temperature and
pressure contain equal numbers of particles
Molar volume = the volume one mole of gas occupies
at 0oC and 1.0 atm pressure
One mole of any gas will occupy 22.4L
Practice Problem
Calculate the volume that 2.0 Kg of methane gas
(CH4) will occupy at STP
Ideal Gas Law
Ideal gases have almost no volume and the particles
are far enough apart to not exert any type of repulsive
or attractive force on another particle.
Do not exist in real world, but most gases behave like
ideal gases at STP
PV=nRT
Practice
Calculate the number of moles of gas contained in a
3.0L vessel at 3.00 x 102 K with a pressure of 1.5 atm
PV = nRT
P = 1.5 atm
V = 3.0L
R = .0821
T = 3oo K
N=?
Gas Stoichiometry
Remember, coefficients represent the number of moles
of a reactant or product
2 C4H10 + 13 O2 8 CO2 + 10 H2O
Calculations involving only volume
CH4 + 2 O2 CO2 + 2H2O
It takes 2 liters of oxygen to react with 1 L of methane
to produce 1 liter of carbon dioxide and 2 liters of water
Volume to volume problem
What volume of oxygen gas is needed for the complete
combustion of 4.0 L of propane gas (C3H8)? Assume
constant pressure and temperature.
C3H8 + 5O2 3CO2 + 4H2O
Start with what you know: 4.0L C3H8
2. What is the ratio of Oxygen to propane? 5 oxygen
1 propane
3. Multiply the amount of propane by the ratio to get
oxygen 5 x 4 = 20 L
1.
Volume to Mass Problem
Ammonia is synthesized from hydrogen and nitrogen
gases. N2 + 3H2 2 NH3
If 5.00 L of nitrogen reacts completely by this reaction
at a constant pressure and temperature of 3.00atm and
298K, how many grams of ammonia are produced?
1. Analyze problem (V, P, T, )
2. Solve for unknown
Determine volume ratio
Use ratio to determine liters of ammonia produced
Rearrange and use ideal gas law to solve for n (use liters
of ammonia produced as V)
3. Convert moles of ammonia to grams of ammonia