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States of Matter - Coggle Diagram
States of Matter
Intro
IMF (Inter molecular force)
Types
Dipole - Dipole
Hydrogen
Special type of dipole dipole
Properties
Act among permanent dipoles
Ends of dipole possess partial charges called delta (<1.6*10^-19)
Weaker than ion-ion force
Interaction energy proportional to
1/r^6 between two rotating polar molecules
1/r^3 in stationary polar molecules
Dispersion/London
Interparticle forces among non polar molecules
Interaction energy proportional to 1/r^6
Strength of this forces depends upon
Molar masss
No of e
Surface area
Dipole-Induced dipole/DEBYE
It operates between molecules having perm dipole as well as lacking one (u=0)
Permanent dipole induces dipole on electrically neutral dipole
Interaction energy proportional to 1/r^6
Matter exists in different states based on particle arrangement and energy.
Thermal Energy
Measure of avg kinetic energy of particles
Energy of body arising from the motion of atoms and molecules
Types
Gaseous state
Intro
Measurable properties
Volume
1 L = 1m^3
1 ml = 1cm^3
Pressure
1 atm = 1.01325 bar = 1.01325 * 10^5 Pa
1 bar = 10^5 Pa
Atmospheric pressure
1 atm = 76 cm = 760 mm = 760 torr
P = hdg
mass
Temperature
Celsuis
Farheneit
100 C = 180 F
F = 9/5 C + 32
Kelvin
K = C +273
Thermodynamic scale of temp
Pressure Measuring devices
Barometer
P = hdg
Manometer
Open ended
Description
Concists of U shaped tube with short and long arm
Short limb connected with the vessel containing gas. It measures gas pressure
Long limb is open and subject to P(atm)
Cases
Level of Hg in 2 limbs are equal then gas pressure = P(atm)
Hg of longer limb > Hg of short limb; Gas pressure = P(atm) + h cm
Hg of longer limb < Hg of short limb; Gas pressure = P(atm) - h cm
Close ended
Genrally used to measure low gas pressure
Gas exerts pressure on short limb and forces its Hg level down
Gas pressure = Diff in two limbs
Ideal gas
Gas laws (Macroscopic)
Boyle law (PV)
P is directly proportional to density
Graphs
Charles law (V/T)
Also called isobar
V(t) = V0(1 + 0.0037)
Gay Lussacs law (P/T)
Isochore
Avogadro law (Volume mole)
Under constant temp and pressure
Ideal gas equation
Derivation
R
In SI unit
8.31 J/K mol
L atm
0.0821
L bar
0.0831
In calorie
2 cal/K mol
L mm
62.3
Standard Conditions
STP
1 atm
T = 0C V = 22.4 L
1 bar
T = 0 C; V = 22.7 L
SATP
1 atm
T = 25C; V = 24.4 L
1 bar
T=25 C; V = 24.7 L
PV = nRT
Variations and Applications
Density form
d = PM/RT
Work done by expamsion/compression gas
Kinetic Theory Explanation of Ideal gases (microscopic)
Postulates
Mathematical formulation
Molecular speed distributions
Equipartition of energy
Mixtures of gases
Daltons law of Partial pressure
Intro
Describes relation between pressure of mixture of non reacting gas and individual pressures
P(t) * X1 = P1
Partial pressure = Mole fraction * total pressure
Applications
Aqueous Tension and Dry gas
P(dry gas) = P(observed/moist gas) - P(water vapour)
Relative Humidity = Partial pressure of water in air/ Aq tension
Grahams law
Intro
Used to compare the movement of different gases.
Types of gas movemnt
Diffusion
Effusion
Formula
Constant temp and presuure
Inversly proportional to density and Molecular weight
r1/r2 = Volume diffused by time taken = moles diffused/time taken = pressure dropped/time taken = 1sqrt./density = 1/sqrt.Mw
Const temp pnly
r1/r2 = P1/P2 *sqrt. Mw2/Mw1
Const pressure only
r1/r2 = sqrt. (T1/ T2 * Mw2/Mw1)
Applications
Enrichment /isotopic seperation factor
f = Final molar ratio/ Initial molar ratio
Amagat's law
Same as dalton but for volume
Partial volume of gas = Mole fraction * Total volume
Real gas
Introduction
Molecular collisions
Liquefaction
Vander walls equation
Other equations