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Chem 106 > Final Review > Flashcards

Final Review Flashcards

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1
Q

kinetic molecular theory

A

explains the behavior of gases based on the motion of their particles

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2
Q

what is a gases average kinetic energy proportional to?

A

absolute temp

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3
Q

what changes a gases volume?

A

temp and pressure

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4
Q

effusion

A

gas leaking through small holes from a high pressure area to a low pressure area

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5
Q

u

A

speed of molecules

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6
Q

smaller mass=

A

higher speed

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7
Q

absolute temperature

A

temp expressed on the Kelvin scale whose zero value is absolute zero

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8
Q

ideal gas

A

gas whose behavior is predicted by the linear relations defined by the combined gas law

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9
Q

STP Temp

A

273K

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10
Q

STP Pressure

A

1 atm

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11
Q

at STP, 1 mol of gas has a volume of…

A

22.4 L

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12
Q

molar volume=

A

v/n

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13
Q

density of gas

A

MP/RT

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14
Q

low molar mass means…

A

low density

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15
Q

what remains constant according to Boyle’s law?

A

temp and number of moles

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16
Q

what remains constant according to Charles law?

A

pressure and number of moles

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17
Q

what remains constant according to Amontom’s law?

A

volume and number of moles

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18
Q

what is constant according to the combined gas law?

A

number of moles

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19
Q

partial pressure

A

pressure of individual gases in a mixture

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20
Q

what finds partial pressure?

A

P1=xPtotal

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21
Q

what is the solubility of gases dependent on?

A

temp and pressure

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22
Q

as solubility increases…

A

pressure increases

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23
Q

as solubility decreases…

A

temp increases

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24
Q

what affects vapor pressure in liquids?

A

temp and intermolecular forces

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25
vapor pressure
pressure exerted by a gas in equilibrium with liquid
26
what r do you use in the Clausius-clapeyron equation
8.3145
27
what does normal mean?
1 atm
28
how do you find total vapor pressure?
mole fraction * partial pressure
29
colligative properties
set of properties of a solution relative to the pure solvent
30
what do colligative properties depend on?
concentration of solute particles not identity
31
what is molality?
moles/kg of solvent
32
how does lattice energy affect solubility?
large lattice energy means limited solubility
33
volatile
having a significant vapor pressure at a given temp
34
what is the vapor pressure at a liquids normal boiling point?
1 atm
35
when is a liquid more volatile?
when it has a higher vapor pressure
36
why are theoretical and experimental values on van't Hoffs factor different?
cations and anions cluster together and act as one molecule, this causes the fpd and bpe to be less than predicted
37
osmotic pressure
pressure applied across a semipermeable membrane to stop the flow
38
what does the kinetic molecular theory assume about gases?
1. they have a small volume 2. they dont interact with other gas molecules 3. move randomly and constantly 4. engage in elastic collisions 5. average kinetic energy is equal to absolute temp
39
does one torr equal one mmHg?
ya
40
what affects vapor pressure
temp, surface area, intermolecular area and solute
41
can gas be soluble in water if the gas is non polar?
yea
42
is the pressure of a gas inversely proportional to its temperature in kelvin?
no
43
in a spontaneous process, what will always increase?
entropy of the universe
44
what doesn't lead to an increase in entropy?
decreasing the volume of a gas
45
the pressure of a gas is inversely proportional to...
volume of the gas
46
according to Avogadro's thing, equal volumes of gas under the same temp and pressure have equal what?
number of particles
47
the density of a pure gas at STP depends on its
molar mass
48
is the boiling point of pure water always at 100*C?
no you stupid bitch
49
what are colligative properties dependent on?
relative numbers of solute and solvent particles in a solution
50
what doesn't cause a system to shift to the right?
change in volume (decrease)
51
pure water at any temp has
[H3O]=[OH]
52
is HNO3 a strong acid?
yes dumbass
53
the degree of ionization of a weak acid
varies with concentration and depends on Ka value
54
if K>Q, will the reactants concentration decrease or increase?
decrease dumb bitch
55
reduction
gains electrons
56
oxidation
loses electrons
57
reducing agent
species that is oxidized
58
oxidizing agent
species that is reduced
59
the more positive E is...
the greater the probability that it will be reduced (wants to be reduced)
60
anode
electron at which oxidation takes place (-)
61
cathode
electron at which reduction takes place (+)
62
what's on the left of a cell diagram
anode
63
whats on the right of a cell diagram
cathode
64
driving force behind a spontaneous reaction?
motional freedom of particles increasing
65
when in a process always spontaneous?
change in H<0 and change in S>0
66
micro states
distribution of particles among energy levels
67
enthalpy
change in heat (H)
68
entropy
how dispersed energy is (S)
69
three types of motion
rotational, translational, vibrational
70
integrated rate law
change in concentration of a reactant with time
71
units for 0th order
M/s
72
units for first order
1/s
73
units for 2nd order
1/Ms
74
what is energy distribution affected by?
molecular motion and volume
75
what remains constant with Gibbs free energy?
temp and pressure
76
what does a reaction rate depend on?
concentration
77
if something is spontaneous what is the change in G of the system equal to?
less than 0
78
equilibrium constant
K
79
what does a large K value mean?
reaction is product-favored
80
what does chemical equilibrium mean?
forward rate=reverse rate
81
what happens when Q>K?
reaction occurs in the reverse direction
82
what happens when you change the volume of a gas in a reaction?
change the partial pressure
83
what does a decrease in the volume/increase in pressure move the reaction towards?
side with the lower number of moles
84
what does an exothermic reaction move the reaction towards?
reactants
85
what does an increase in temp do to the direction of a reaction?
forwards
86
what are strong acids converted to in water?
H3O
87
the more oxygen atoms...
the stronger the acid
88
pH buffer
weak acid and conjugate base
89
when can the common-ion affect be applied?
anytime there's a buffer
90
equivalence point
equal # of moles of acid and base
91
molar solubility symbol
S
92
molar solubility units
mol/L
93
solubility units
g/L or mg/L
94
Q>K
precipitate forms

Chem 106 (13 decks)

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