Robert Boyle
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Discovered by… that guy! 
Describes the inverse
relationship between the
pressure and volume of a
gas, if the temperature is
kept constant in a vacuum.
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How to Solve…
 Label all values (Pressure= P,
Volume=V)
 Write base formula
 Substitute variables with given
information
 Solve for unknown value
Discovered by that other guy 
At constant pressure, the volume
of a gas increases/decreases at the
same rate as it’s temperature (the
Kelvin scale, convert from Celsius).
 Can be written in 3 different ways
 How to solve…
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 Label all given values (V=Volume,
T=Temperature in Kelvin)
 Set up base equation (see formulas).
 Substitute variables for values
 and solve.
Jacques
Charles
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Discovered by another guy 
The pressure of a gas is directly
proportional to the gas's
temperature.
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How to Solve
 Same as the other two!
 Label given information
(P=Pressure, T=Temperature)
 Set up base formula
 Substitute for given values
 Solve for unknown
Joseph Louis
Gay-Lussac
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Combines the previous three Gas Laws into one.
The ratio between the product of pressure and volume of a gas
and it’s temperature remains constant.
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How to solve…
 If you paid any attention to the last three slides, you should already
know.
 P=Pressure, V=Volume, T=Temperature
Gasses are made up of tiny particles
(atoms/molecules) with immense distances
between them.
 Gas particles are in constant, random motion and
often collide with each other, with pressure being
the result of this.
 Molecular collisions are elastic, meaning that
despite individual molecules gain or lose kinetic
energy, the collisions don’t affect the whole gas
sample’s kinetic energy.
 At a given temperature, molecules in a gas
sample have a range of kinetic energies, however
the average remains constant and as the
temperature increases, so does the average
velocity and kinetic energy of the gas sample as a
whole.
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Ideal Gases are those which adhere to all
predictions made in the Kinetic Molecular
Theory.
Usual atmospheric conditions produce Ideal
Gases.
At very high pressures or very low
temperatures, gases do not behave ideally,
these resulting in physical changes to the
gas.
At very high pressures, gases can condense
into solids.
At very low temperatures, molecular
attractions become weak and the gases
become liquefied.
These state of matter changes do not affect
the gas’s original chemical composition.
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Standard Temperature and Pressure
Used in Gas Laws as the ideal values for all
gases
Standard Temperature = 0°Celsius, or 273 Kelvin
Standard Pressure:
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1 atm
101.3 kPa
760 mmHg
760 torr
Discovered by yet another dead guy! 
Equal volumes of gases at the same
temperatures and pressures contain the same
number of molecules.
 1 mol of any gas occupies 22.4 Liters at STP.
 Coefficients in chemical equations can
Amedeo Avogadro
represent moles, molecules, and volumes of
the reactants or products.
 Equations can be…
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Mole to Mole
Volume to Volume
Moles to Volume
All require factor-label method
Dan Jugo and Ryan Spoltore
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Organic Molecule- an organic molecule
contains carbon and hydrogen
▪ Examples: carbohydrates, proteins, and lipids
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Inorganic Molecules- inorganic molecules
have either one or no carbon or hydrogens
▪ Examples: water, carbon dioxide (exception)
Crude oil has components with different
boiling points.
 The components are heated and their vapors
are passed into a column.
 The vapors go from high to low
 Components of higher boiling points
condense and return to the solution
 Components of lower boiling points pass
through the column and are collected.
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Density is mass/volume
Density is affected by the number carbon atoms present in
the solution
As we learned in the Viscosity Lab when there are more
carbons the density of the solution is higher
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Hydrocarbons- molecular compounds that
contain atoms of the elements hydrogens
and carbons
Small hydrocarbon molecules (contain 1-4
carbons) have low boiling points because the
are only slightly affiliated with each other or
to other petroleum molecules
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Meth- 1 carbon
Eth- 2 carbons
Prop- 3 carbons
But- 4 carbons
Pent- 5 carbons
Hex- 6 carbons
Hept- 7 carbons
Oct- 8 carbons
Non- 9 carbons
Dec- 10 carbons
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Alkane- identify alkanes by ending: -ane
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Saturated
Single bonds
Formula for linear alkanes: CnH2n + 2
Formula for branched alkanes: CnH2n + 2, n > 3
Fewer number of carbons, the lower the intermolecular
forces; thus, the lower the boiling point
 Greater number of carbons, the greater the surface area
 The more carbon atoms, the higher the viscosity.
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Example: Ethane
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Alkene identified by -ene ending
 Unsaturated
 Single bonds with at least one double carbon to
carbon bond
 Have a higher boiling point than alkanes because
a double bond is stronger than a single bond.
 Due to the double bonds, the substances are less
viscous
 Surface area is less than alkanes
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Alkynes- end in –yne
 Unsaturated
 At least one triple bond between carbons
 Higher boiling points than alkanes or alkenes
 Due to triple bonds alkynes are less viscous than
alkenes
 Surface area even less due to triple bonds
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Same number of carbons and hydrogens, just
varying structure
Isomers all have the same chemical formula
When a number appears before the
hydrocarbon that identifies where the double
or triple bonds are located
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Branched chain- made from carbon atoms
where at least one carbon atom is joined onto
more than two other carbon atoms. Lower
boiling points than straight chains.
Straight chain- made from carbon atoms
joined onto no more than 2 other carbons
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Molecular Formula shows the number of
carbons and hydrogens but not the structure
or electrons.
C4H10
Butane
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Structural shows where the carbons and
hydrogens are located and the types of bonds
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Dot diagrams show where the electrons are
between each carbon and hydrogen and also
the types of bonds
H HHH
HC C C C H
H HHH
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When monomer molecules are combined to
create a polymer