Assignment 6 Flashcards by Tyler L

properties of a gas

volume

density

mass/amount/moles

pressure

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IMFs (what do they determine)

determine physical properties

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Particle Theory/Kinetic Molecular Theory

particles…

are meaured in moles (6.02 x 10²³)

have mass

are the smallest representative unit of a substance that contain the properties of the larger substance

travel randomly in a straight line

speed indicate its heat

have no IMFs (ideal gas assumption)

collide with each other and the walls of the container (measured by vol and pressure)

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particles

the smallest representative unit of a substance that contains the properties of the larger substance

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ideal gas assumption

no IMFs

PV = nRT

theoretical

no freezing/boiling point

no energy (heat) lost

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Relationship of Pressure to Volume

Inverse

same # particles + more volume/space = less bumping of particles = less pressure

same # particles + less volume/space = more bumping = more pressure

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Relationship of Pressure to Temperature

Direct (if you start at absolute zero)

more temp = more movement of particles = more bumping = more pressure

less temp = less movement of particles = less bumping = less pressure

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Relationship of Temperature to Volume

Direct (if you start at absolute zero)

more temp = more motion = more collision = more push on conainer = more volume

less temp = less motion = less collision = less push on conainer = less volume

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Relationship of Number of Moles (n) to Pressure/Temperature/Volume

Direct

more moles = more mass = more vol

more moles = more particles in same space = more bumping = more pressure

more moles = more particles bumping = more KE/heat = more temp

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Proportionality Constant R =

0821 (for atm)
314 (for kPa)
396 (for mmHg/torr)

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what happens as a system is cooled

density increases

kinetic energy (temp) decreases

pressure decreases

volume decreases

particles squish together (IMFs became important, no ideal gas assumptions no equations)

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solid

low KE

IMFs > KE of particles

incompressable

maintains shape and vol

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liquid

medium KE

IMFs ≈ KE of particles

incompressable

constant vol, variable shape

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gas

high KE

IMFs (essentially zero) < KE

compressable

no set vol or shape

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boyle’s law

P₁V₁ = P₂V₂

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charles’ law

V₁/T₁ = V₂/T₂

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Gay-Lussac’s Law

P₁/T₁ = P₂/T₂

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gas law equation for descriptive and changing moles

PV = nRT

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gas law equation for changing conditions, constant moles

P₁V₁ P₂V₂

———— = nR = ———-

T₁ T₂

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mole fraction equation

P_x n_x

—————— = —————–

P_TOTAL n_TOTAL

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PV = nRT

gas law equation for descriptive and changing moles

P₁V₁ P₂V₂

———— = nR = ———-

T₁ T₂

gas law equation for changing conditions, constant moles

density (at STP) =

gfm

22.4

density (not at STP) =

P(gfm)

Dalton's Law of Partial Pressures

sum of the pressures in a vessel for a mixture of gases depend only on the pressures of the individual gases P_TOTAL = P₁ + P₂ + ... + P_n

Graham's Law (of Diffusion and Effusion)

smaller things diffuse faster

diffusion

particles move from high concentration to low concentrations until they are equal

effusion

particles will move from a pressurized space to a non-pressurized space (vaccum)

temperature

measure of avg kinetic energy

STP

standard temp (0ºC/273K) and pressure (1atm/101.3kPa/760mmHg/760torr)

vapor

small airborne particles of liquid (not molecules like gas) intermediary between gas and liquid gas where liquid phase is present

dynamic equilibrium

evaporation rate = condensation rate

evaporation

no external energy added automatically occurs with any liquid

vapor pressure

partial pressure of vapor above any liquid temp dependent: higher temp = higher avg KE = more particles have ability to leave = higher vapor pressure

boiling

P_TOTAL = P_VAPOR atmospheric pressure = vapor pressure

freezing

phase change from liquid to solid

melting

phase change from solid to liquid

condensation

phase change from gas to liquid

vaporization

phase change from liquid to gas

sublimation

phase change from solid to gas without passing through liquid

desposition

phase change from gas to solid without passing through liquid

triple point

temp and pressure where all phases (solid, liquid, gas) occur simultaneously

equilibrium

the temp and pressure where two phases exist simultaneously

critical point

temp above which the substance is always a gas

when do ideal gases behave like actual gases

at high temp/volume or low pressure

1 atm =

101.3 kPa = 760 mmHg = 760 torr

2 bonds + electron pairs

linear sp

3 bonds + electron pairs

trigonal planar sp²

4 bonds + electron pairs

tetrahedral sp³

5 bonds + electron pairs

bipyramidal sp³d

6 bonds + electron pairs

octahedral symmtery sp³d²