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Chemistry > The Gas Phase > Flashcards

The Gas Phase Flashcards

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1
Q

Gases are classified as fluid because they…

A

can flow into and tke the shape of whatever container

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2
Q

Gasses are different from liquids as…

A

very low intermolecular forces between gas particles

molecules move very rapidly and are far apart

and compressible

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3
Q

1 atm =

A

760 torr

760 mmHg

101.325 kPa

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4
Q

Sphygamomanometers

A

medical devices which meaure blood pressure

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5
Q

How Barometers Work

A

atmospheric pressure creates downward force on mercury which exerts upward force creating a vacumn

when air exerts greater force than weight of mercury, it goes up

when air exerts lesser force than weight of mercury, it goes down

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6
Q

STP vs Standard State

A

1 atm 273 K

1 atm, 273K , 1 M

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7
Q

Ideal Gas

A

a gas whose molecules have no inter molecular forces and occupy no volume

real gases deviate from this at high/low pressures (low/high volumes)

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8
Q

Ideal Gas Law

A

PV=nRT

R = 8.21*10^-2

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9
Q

Ideal Gas Law With Density

A

p = m/V = PM/RT

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10
Q

Combined Gas Law

A

used to relate changes in temperature, volume and pressure.

P1V1/T1 = P2V2/T2

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11
Q

Determining Molar Mass of Gas at STP

A

1) Determine mass of sample at the given temp/pressure
2) Find density of sample given the volume
3) find volume at STP using combined gas law and STP conditions
4) Density at STP is sample mass divided by volume at STP found
5) find molar mass by multiplying the density calculated and volume of STP of 1 mole gas ( 22.4 L/mol)

mm = p STP * 22.4 L/mol

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12
Q

Avogadro Principle

A

all gases at constant temperature and pressure occupy volumes that are directly proportional to the number of moles of gas present

n/V = k or n1/v1 = n2/V2

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13
Q

Boyles Law

A

P1V1 = P2V2 pr PV = k

gas sample held at constant temperature (isothermal) volume is inversely proportional to its pressure

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14
Q

Boyles Law Isothermal Compression

A

As pressure increases, volume decreases

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15
Q

Charles Law

A

at constant pressure (and moles), the colume of a gas is proportional to its temperature in kelvin

V1/T1 = V2/T2

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16
Q

Charles Law (Isobaric Expansion)

A

as temperature increases, so does volume

17
Q

Gay-Lussacs Law

A

likes Charles but relates pressure and temperature where volume and moles are constant

P1/T1 = P2/T2

18
Q

Gay-Lissacs Law (Isovolumetirc Heating)

A

as temperature increases, so too does pressure

19
Q

When two or more gases that do not chemically interact are in one vessesl they will _______. Therefore the pressure exerted by each gas is equal to the pressure that the gas would exert if _____ Pressure exerted by each gas is known as a ______

A

behave independently of each other

it were the only one in the container

partial pressure

20
Q

Daltons Law of Partial Pressures

A

Total pressure of gasseous mixture is equal to the sum of all partial pressures

PT = Pa+Pb+Pc+….

21
Q

Mole Fractions and Partial Pressures

A

Pa = Xa * PT

Xa = moles of a / total moles of gas

22
Q

Vapor Pressure

A

pressure exerted by evaporated particles above the surface of a liquid

the concentration of a gas in liquid can change depending on the applied pressure

[a] =kH * Pa or [a1]/P1 = [a2]/P2 =kH

kH = henrys constant

[a] = concentration of gas

23
Q

Assumptions of Kinetic Molecular Theory

A

1) gases are made of particles with volumes negligible to container volume
2) gas atoms/molecules have no intermolecular forces
3) gas particles have random motions
4) collisions between any two gas particles are elastic (concervation of momentum and KE)
5) avg kinetic energy is proportional to temperature of gas

24
Q

Avg Gas Kinetic Energy

A

KE = 1/2mv^2 = 3/2kBY

kB = Boltzmann Constant (1.38*10^-23)

speed of moleculae is propotional to its temperature

25
Q

Avg Gas Molecular Speeds

A

Root-mean square speed

= sqrt ( (3RT)/mm )

R = ideal gas constant 
mm = molar mass
26
Q

Maxwell-Boltzmann Distribution Curve

A

curves of molecular speed of gas molecules at different temperatures

as temp increases, number of molecules at faster speeds increases

27
Q

The kinetic molecular theory of gasses predicts that ____ gases diffuse more _____ than ____ ones due to differing avg. speeds. This is because all gas particles have same avg. KE at same temperature.

A

heavier

slowly

lighter

28
Q

Grahams Law

A

r1/r2 = sqrt( mm2/mm1)

under isothermal and isobaric conditions, the rates at which two gases diffuse are inversely proportional to the sqrt of their molar masses

29
Q

Effusion

A

flow of gas particles under pressure from one compartment to another through a small opening

30
Q

Real gases deviate from ideal gas behavior to some extent when gas atoms/molecules are _____ under high pressure at low volume or low temperature.

A

forced into close proximity

31
Q

At extremely high pressures, size of particles become _____ compared to distance between them so a LARGER volume is taken up and ____ can never be met.

At moderately high pressure, a gas volume is _____ than predicted ideal gas law due to intramolecular attraction

A

relatively larger

0

less

32
Q

As the ______ pressure for a given temp is approached, _____ forces become more significant until the gas ____ into a liquid.

A

condensation

intramolecular

condenses

33
Q

As the temperature of a gas _____, the avg speed of a gas decreases and the attractive forces become ____

A

decreases, significant

34
Q

The closer a gas is to its ______ point, the less ideally it acts. It will have a ____ volume than predicted.

At extremely low temperatures , gas will occupy ______ space than predicted

A

boiling point, smaller

more

35
Q

van der Waals Equation of States

A

(P + (N^2 a)/V^2) (V-nb) = nRT

a and b are physical constants experimentally determined

a - attractive forces between molecules (larger polar ones have high value)

b - volume of molecules themselves

Chemistry (9 decks)

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