Unit 3 Flashcards

1
Q

Kinetic Molecular Theory

A

Describes Ideal Gas No Attractive Forces

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2
Q

Boyles Law

A

Inverse relationship of pressure and volume P1V1=P2V2

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3
Q

Charles Law

A

Proportional relationship of temperature and volume V/T=V/T

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4
Q

Combined Gas Law

A

No direct relationships PV/T=PV/T

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5
Q

Avogadros Law

A

Amount/Volume Relationship If two gases have same temp & pressure, must have same # of molecules

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6
Q

Daltons Law

A

If you have mixture of gases, the sum of all the pressures of the gases equals total pressure of mixture

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7
Q

Use % to find Partial Pressure

A

Mole percentage of gases overall makeup is proportinoal to percentage it contributes to overall pressure

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8
Q

Effusion

A

r1/r2=m2/m1

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9
Q

Root Means Square

A

Assumes molecule possess avg. kinetic energy Urms= SqrRt(3RT/M)

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10
Q

Ideal Gas Law

A

PV=nRT

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11
Q

Ideal Gas Law (for Density/Molar Mass)

A

M=dRT/P

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12
Q

Van Der Waals Equation

A

Tweaks ideal gas law for attractive forces a & b are constants for each molecule P=(nRT/V-nb)-(n2 a/ v2)

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13
Q

1 mol of an gas @ STP

A

Equals 22.4L

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14
Q

Mass-Volume Stoichometry

A

Mass Given -> Moles Given -> Mols of Unknown -> Volume of Unknown

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15
Q

Solute

A

Substance being disolved

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16
Q

Solvent

A

Does the disolving

17
Q

Soluble

A

Able to be dissolved

18
Q

Insoluble

A

Cant be dissolved

19
Q

Like Dissolves

20
Q

Suspensions

A

needs to be constantly stirred or solute particles will settle out Can be filtered out easily

21
Q

Colloids

A

Mixture that appears to be solution, but will eventually settle out Test with Tyndall Effect (shinning light)

22
Q

Liquid-Gas Solution Factors

A

Temperature and Pressure

23
Q

Most are soluble

A

Nitrate Salts

Alkali Metal Salts

Ammonium Salts

Halogen Salts (except lead. mercury, silver)

Sulfate Salts (except lead, mercury, barium, calcium)

24
Q

Molarity

A

Moles Solute/Liters Solution

25
Molality
Moles Solute/Kilogram Solvent
26
Mass Percentage
mass component/mass solution x100%
27
ppm
mass component/mass solution x10^6
28
ppb
mass component/mass solution x10^9
29
Volatility
volatile substances evaporate quickly
30
Four Colligative Properties
Vapor Pressure Reduction Boiling Point Elevation Freezing Point Depression Osmotic Pressure
31
Boiling Point Elevation
[Delta]Tb=Kb x m Constant is .52 c/m
32
Freezing Point Depression
[Delta]Tf=Kf x m Constant is 1.86 c/m
33
Osmotic Pressure
[Pie Symbol?]=MRT
34
Isotonic
When two solutions of indentical concentrations are separated
35
Hypotonic
One solution os lower than others
36
Hypertonic
One solution is higher than other