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CHEM > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

Pressure

A

Force/unit area or ma/area or P=dh*g

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2
Q

1atm

A

=760mmHg=760torr=1.01*10^5pascals

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3
Q

atmospheric presure

A

Gas molecules exert presure on their surroundings

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4
Q

barometer

A

measures atmospheric pressure; a long tube is filled with mercury and turned upside down a dish filled with mercury. The height difference or the height of how much mercury is in the tube is the atmospheric pressure.
Outside pressure pushing liquid up the tube.

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5
Q

manometer

A

is another pressure measuring device used to measure pressures close to atmospheric pressure.

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6
Q

open tube manometer

A

there is mercury in the tube between gas and atmospheric pressure.

When gas in the tube pushes harder, Pgas>patm, Pgas=patm+∆h

When the atmospheric pressure pushes harder on the mercury in the tube than the gas pressure, Pgas<Patm, Pgas=patm-∆h

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7
Q

2 gases, densities given

A

dhg=dhg; solve for height. then use +or-∆H equation

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8
Q

Ideal gas behavior when

A

1) low external pressure 2) high temperature

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9
Q

Boyle’s law

A

PV=PV

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10
Q

Charle’s Law

A

V/T=V/T

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11
Q

Amonton’s Law

A

P/T=P/T

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12
Q

Avogadro’s Law

A

V/n=V/n

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13
Q

General gas law

A

PV/T=PV/T

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14
Q

Gas law inverse/directly proportional

A

Variables on same side=inversely proportional; opposite sides=directly proportional

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15
Q

Gases are said to mix

A

no reaction

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16
Q

ideal gas law

A

PV=NRT

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17
Q

Ideal gas law variables

A

pressure in atm, v in liters, R=0.0821, T in K (C+273)

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18
Q

rewrite ideal gas law for density and molar mass

A

d=m/v=P(MM)/RT; MM=dRT/P

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19
Q

P and T are constant

A

V is directly proportional to moles.

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20
Q

V and T are constant

A

P is directly proportional to moles.

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21
Q

STP

A

273K and 1atm

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22
Q

1 mole of gas at STP

A

22.4 Liters.

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23
Q

Partial pressure

A

mole fraction*P total. mole fraction moles of gas/total moles of the entire gas

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24
Q

Collecting gas over water

A

Ptotal=Pgas+Pvp of H20

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25
Q

Effusion

A

ability of moleculues to flow from a container through a hole to teh outside world or into another container

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26
Q

Gas weight effusion

A

heavier the gas, the slower the effusion rate; the lighter the gas, the faster the effusion rate.

Heavy gas-more time
lighter gas-less time

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27
Q

Graham’s law

A

rate of effusion of gas2/rate of effusion of gas1=square root of mm of gas 1/square root of mm of gas 2= time of effusion of gas 1/time of effusion of gas 2.

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28
Q

Kinetic molecular theory

A

behavior of gases at the atomic level

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29
Q

3 postulates of kinetic molecular theory

A

particles of gases separate much larger than their size (fill the room), particles in constant motion, collisions do not lose energy, total energy=kinetic energy, average kinetic energy is dependent on temperature regardless of their molar masses.

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30
Q

gas is the same termperature

A

average ke is same for all gases.

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31
Q

incresing pressure

A

increases the average kinetic energy

32
Q

kinetic energy equation

A

=1/2m*u^2
m=mass in kilograms
u=speed or velocity in m/s

33
Q

root mean square speed/velocity or rms

A

rms velocity= square root of (3RT/MM)

34
Q

Van Der Waals equation

A

for real gases

35
Q

correction for intermolecular forces

A

observed gas pressure should be less than the gas pressure predicted. Moleculues in the gas help lessen the force of the gas.

36
Q

correction for molecular volume

A

finite sizes; the highest value for b should be molecules that are the largest molecules

37
Q

At high external pressures

A

PV/RT lower than ideal-intermolecular attraction; higher values due to molecular volume.

38
Q

Heat of fusion

A

energy needed by a substance to transfer from solid state to liquid phase. melting

39
Q

fusion=

A

-freeze (liquid state to solid)

40
Q

heat of vaporization

A

liquid to gas state energy. boiling

41
Q

vap=

A

-condense. gas to a liquid state.

42
Q

solid to liquid to gas

A

heat is absorbed or gained.

43
Q

gas to liquid to solid

A

heat is liberated or released.

44
Q

temperature change/diagonal line

A

q=mc∆T

45
Q

phase change, horizontal line

A

q=m∆h here m is moles or mass

46
Q

Triple point

A

s, l, g coexist

47
Q

critical point

A

g and l phases are indistinguishable; also supercritical fluid

48
Q

if the slope of the line between the liquid and solid phase is leaning toward the liquid,

A

solid has a higher density

49
Q

if the line is leaning toward the solid

A

solid has a lower density than the liquid.

50
Q

line that creates the equilibrium between the liquid and gas phase

A

ccreated by the clausius-clapeyron equation

51
Q

normal melting point

A

point where a solid melts at 1.0 atm

52
Q

normal boiling point

A

liquid boils at 1.0atm

53
Q

normal sublimation point

A

where a solid sublimes at 1.0 atm

54
Q

if the pressure at the triple point is > 1.0 atm

A

then the substance does not have a not have a normal boiling point or a normal melting point; it does have a normal sublimation point

55
Q

Vapor pressure

A

amount of pressure in a sealed container that is helping a solution, a liquid or a solid, turn into the gas phase

56
Q

point on the solid-liquid equilibrium line

A

point where hte liquid is boiling. the bapor pressure of liquid=pressure of the gas.

57
Q

Clausius-claperyron equation

A

explains curve of the liquid/gas equilibrium.

On formula sheet. t must be in kelvin. ∆Hvap in KJ and R (8.314–gas lawconstant with energy) is in J, so convert.

58
Q

forces in order of strength

A

ion/ion, hydrogen bonding, dipole/dipole, london/dispersion

59
Q

h bonding

A

NOF

60
Q

increase the IMF, increase

A

increase the BP, FP/MP and ∆H

61
Q

same IMF’s for covalent

A

higher the molar mass, higher the BP, FP, and∆H

also the more linear it is.

62
Q

same IMF’s for solid ionics,

A

higher the charge, the greater hte IMF. same charge, the smaller anion has the stronger imf.

63
Q

stronger the IMF, surface tension

A

surface tension is greater

64
Q

water molecules

A

4 h bonds with neighbors. accounts for high surface tension, high capillarity and high heat of vaporization.

65
Q

surface tension

A

energy to increase the surface areaa by a unit amount

66
Q

capillary action

A

ability of a liquid to rise or fall in a container

67
Q

cohesive forces

A

hold liquids together

68
Q

adhesive forces

A

forces between liquid and a solid surface.

69
Q

higher viscosity

A

stronger attracted moleculue with the longest chain. resistance of liquids to flow

70
Q

vapor pressure

A

depends on Temperature.

71
Q

higher the VP

A

the lower the BP

72
Q

polarization

A

process of inducing a dipole

73
Q

polarizability

A

relative tendency of a charge distribution to be distored from its normal shape by an external electric field

74
Q

higher the molar mass

A

the greater the polarizaibility

75
Q

same molar mass

A

more e-, then more polarizability.

CHEM (5 decks)

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