# Dalton`s Law Ideal Gas Law Graham`s Law

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SEMESTER REVIEW QUIDE FOR MRS. EUBANKS’ CHEMISTRY 1
TEST: BRING TO TEST FOR GRADE AND HELP SHEET
Boyle’s Law
For a given mass of gas at
constant temperature, the
volume of a gas varies
inversely with pressure
Charles’ Law
The volume of a fixed
mass of gas is directly
proportional to its
Kelvin temperature if
the pressure is kept
constant.
Guy-Lassac's Law
Combined Gas Law
The pressure of a gas is
directly proportional to the
Kelvin temperature if the
volume is kept constant.
Combines Boyle’s, Charles’, and the
Temperature-Pressure relationship into
one equation. Each of these laws can be
derived from this law.
PV = k
V1 T2 = V2 T1
P 1 T 2 = P 2 T1
V 1 P 1 T 2 = V2 P 2 T 1
P1V1 = P2V2
V1
V2
=
T1
T2
P1
P2
=
T1 T2
P1V1 P2 V2
=
T1
T2
Dalton’s Law
Ideal Gas Law
Graham’s Law
At constant volume and
temperature, the total
pressure exerted by a
mixture of gases is equal
to the sum of the
pressures exerted by each
gas
The Ideal Gas Law relates the
pressure, temperature, volume, and
mass of a gas through the gas constant
“R”.
The rates of effusion/diffusion of
two gases (A and B) are inversely
proportional to the square roots of their
formula masses. [It can be a ratio of
molecular speeds,
effusion/diffusion times, distance
traveled by the molecules , or the amount
of gas effused]
Ptotal = P1 + P2 + P3 + ...Pn
PV = nRT
RateA = √molar massB
RateB = √molar massA
Abbreviations
Atm = atmosphere
mm Hg = millimeters of mercury
Torr = another name for mm Hg or 1.33 Kpa
Pa = Pascal
kPa = kilopascal
K = Kelvin 0C + 273 = K
Standard Conditions
00C = 273 K
1.0 atm = 760.0 mm Hg = 101.325 kPa
STP = 273k &amp; 101.325 kPa
R=0.0821 Latm/molK
R=8.315 dm3kPa/molK
Molecular vs Empirical Formula:
Empirical is reduced to the lowest possible
number for each coefficient if they are all
reducible by the same amount.
Law of Conservation of Mass:
You end up with the same amount you started
with, so equations have to be balanced
∆ = heat is added to an equation
The ideal gas law is an important concept in chemistry.
It can be used to predict the behavior of real gases in
situations other than low temperatures or high pressures.
This collection of ten chemistry test questions deals with
the concepts introduced with the ideal gas laws.
Useful
information:
At STP: pressure = 1 atm = 700 mmHg, temperature = 0
&deg;C
=
273
K
At STP: 1 mole of gas occupies 22.4 L
R = ideal gas constant = 0.0821 L&middot;atm/mol&middot;K or
8.3145cm3/mol&middot;K
Things you need to know:
Reactions Types :use the letter method A,B,C,D
Equations YOU should be able to do: put
examples here to refer back to if needed
Single replacement =
Mole ratios:
Double replacement =
Synthesis or Combination =
Decomposition =
Stoichiometry:
Combustion =
Dimensional Analysis= example
Moles to grams or grams to moles:
Stoichiometry = example
Representative Particles (RP) =amount
Moles to liters or liters to moles:
Gas Molecule Actions &amp; Reactions =
Moles to RP or RP to Moles:
Kinetic Energy (KE) = vocabulary
Atomic Particles and their functions:
Boyle’s Law:
Chemical Bonds form due to:
Charles’ Law:
Ions:
Cation:
Gay-Lussac’s Law:
Anion:
Isotopes:
Electron Configurations: s, d, p, &amp; f blocks:
Combined Gas Law:
Ionic Bonds:
Dalton’s Law:
Covalent Bonds:
Ideal Gas Law:
Diatomic Molecules:
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