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ap chem > unit 5 > Flashcards

unit 5 Flashcards

1
Q

gas properties

A

expand
low density
changes dramatically with a change in pressure/temp
volume, pressure, temperature are interrelated

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2
Q

pressure

A

force exerted per unit area as gas molecules strike the surfaces around them

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3
Q

unit equalities

A
  1. mm Hg = 760. torr = 1 atm = 101.3 kPa = 14.7 psi
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4
Q

mm Hg (millimeters of mercury)/torr

A

atmospheric pressure that can support a column of mercury that is 760. mm high in a barometer

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5
Q

atmospheres (atm)

A

avg. pressure at sea level

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6
Q

pascal (Pa)

A

SI unit of pressure
also expressed as kPa

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7
Q

psi (lbs per square inch)

A

measure of force per unit area

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8
Q

boyle’s law

A

p1v1=p2v2
volume increases = pressure decreases

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9
Q

Charles law

A

v1/t1 = v2/t2
volume increases = temperature increases
always positive

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10
Q

avogadro’s law

A

v1/n1 = v2/n2
volume increases = moles increase

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11
Q

Gay-Lussac’s law

A

p1/t1 = p2/t2
pressure increases = temperature increases

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12
Q

combined gas law

A

p1v1/t1 = p2v2/t2

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13
Q

ideal gas law

A

PV = nRT

P: pressure in atm
V: volume in L
n: moles in mol
R: ideal gas constant (0.08206 when Latm/molK)
T: temperature in K

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14
Q

molar volume

A

volume occupied by 1 mol of a substance

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15
Q

standard temperature and pressure (STP)

A

for gases, molar volume is usually STP (1.00 atm)

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16
Q

density =

A

molar mass / molar volume
molar mass increases = density increases

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17
Q

1 mol of an ideal gas occupies:

A

22.4 L at STP

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18
Q

density of a gas equation

A

d = PM / RT
d: density in g/L
P: pressure in atm
M: molar mass in g/mol
R: ideal gas constant (0.08206 when Latm/molK)
T: temperature in K

19
Q

to find molar mass of a gas:

A

measure mass and volume under known conditions of T and P
use ideal gas law to determine amount of gas in mol
divide mass by moles to get molar mass

20
Q

partial pressure

A

pressure due to an individual component of a gas
Pn = Nn RT/V

21
Q

Dalton’s Law of Partial Pressures

A

sum of partial pressures in a gas mixture = total pressure
P(total) = P(a) + P(b) + P(c)

22
Q

mole fraction (X(a))

A

X(a) = N(a)/N(total)

or

P(a) = X(a)P(total)

23
Q

gas mole fraction

A

percent by volume / 100

24
Q

Vapor pressure

A

gas mixture with partial pressures
temp increases = Vapor pressure increases

25
Q

kinetic molecular theory

A

simplest model for the behavior of gases

26
Q

KMT postulates

A

-negligibly small
-avg. kinetic energy is proportional to Kelvin temp
-collision of one particle with another is elastic

27
Q

pressure =

A

force / area

28
Q

Boyle’s law: proportion

A

volume is inversely proportional to pressure

29
Q

Charles law: proportion

A

volume is proportional to temperature

30
Q

Avogadro’s law: proportion

A

volume is proportional to moles

31
Q

particles of different masses have the (same/different) average kinetic energy

A

same

32
Q

kinetic energy =

A

(1/2)mv^2

33
Q

do lighter particles travel faster than heavier particles?

A

yes

34
Q

temperature and velocity distribution proportion

A

temp increases = higher velocity

35
Q

diffusion

A

gas molecules spread out due to a concentration gradient

-heavier molecules diffuse more slowly

36
Q

effusion

A

gas escapes from a container into a vacuum through a small hole

-heavier molecules effuse more slowly

37
Q

rate is inversely proportional to

A

1 / square root of the molar mass

38
Q

effusion rate a / effusion rate b =

A

square root of molar mass b / square root of molar mass a

39
Q

gases behave ideally when:

A

-volume of gas particles is small compared to the volume between them

-attractions between particles are insignificant

40
Q

finite volume

A

actual size

41
Q

when is finite volume important?

A

high pressure because then the particles occupy a significant portion of the total gas volume

42
Q

when are intermolecular forces important?

A

low temps: collisions occur with less kinetic energy and weak attractions decrease collisions, also causes a decrease in pressure

43
Q

Which postulate of the kinetic molecular theory breaks down under conditions of high pressure?

A

the volume of a gas particle is small when compared to the space between the particles

ap chem (11 decks)

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