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GEN CHEM 2 > Exam 3: ch 19 + 20 > Flashcards

Exam 3: ch 19 + 20 Flashcards

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1
Q

enthalpy

A

heat absorbed or released by a system during a constant pressure process

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2
Q

entropy

A

measure of randomness/disorder in a system

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3
Q

1st law of thermodynamics

A

-energy can not be created or destroyed, but only converted or transferred
-delta E (sys)=q+w

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4
Q

spontaneous process

A

proceeds w/o any outside assistance

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5
Q

reverse of spontaneous

A

nonspontaneous

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6
Q

nonspontaneous

A

proceeds w/ outside assistance only

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7
Q

factors that affect spontaneity

A

temperature and pressure

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8
Q

reversible process

A

system changes so that the system and surroundings can return to original state

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9
Q

irreversible process

A

cannot be undone by exactly reversing the change

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10
Q

are spontaneous process reversible

A

no

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11
Q

is entropy a state function

A

yes

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12
Q

state function

A

actual path is not relevant to final answer

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13
Q

delta S (when given heat and temp.)

A

=q/T

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14
Q

2nd law of thermodynamics

A

the entropy of the universe increases in any spontaneous process

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15
Q

delta S (univ) >0

A

irreversible process, spontaneous

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16
Q

delta S (univ)= 0

A

reversible process

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17
Q

microstate

A

a single possible arrangement of position and kinetic energy of molecules

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18
Q

boltzman equation

A

S=kln(w)

w- # of microstates
k- boltzman constant (1.38 x 10^-23)

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19
Q

more microstates =

A

more entropy

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20
Q

degrees of freedom (DOF)

A

types of motion

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21
Q

translation

A

movement of entire molecule

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22
Q

vibration

A

movement of atoms w/in molecule
(stretching/ contracting of bonds/angles)

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23
Q

rotational

A

movement about an axis

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24
Q

the # of microstates possible increases w/

A

increase of: volumes, temperature, and number of atoms

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25
Q

entropy order of states of matter

A

gas>liquid>solid

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26
Q

when the # of gas molecules increases

A

the entropy of a system increases

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27
Q

delta n > 0

A

increase in entropy

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28
Q

delta n < 0

A

decrease in entropy

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29
Q

entropy of a pure crystalline substance at absolute zero is…

A

zero

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30
Q

enthalpy, entropy, and free energy formation of a rxn

A

products- reactants, use given values multiplied by coefficients

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31
Q

standard entropy for elements

A

zero

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32
Q

entropy unit

A

J/mol x K

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33
Q

enthalpy and fee energy unit

A

kJ/mol

34
Q

delta G =

A

delta H (sys) - (T)(delta S (sys))

35
Q

delta G is negative …

A

spontaneous

36
Q

delta G = 0 …

A

system at equilibrium

37
Q

delta G is positive …

A

nonspontaneous

38
Q

delta G (under any conditions) =

A

delta G (naught) + RTln(Q)

Q-rxn quotient
R- 8.314

39
Q

delta G (naught)=

A

-RTln(k)

40
Q

+ delta H and - delta S

A

+ delta G, nonspont. at all temps

41
Q
  • delta H and +delta S
A
  • delta G, spont, at all temps
42
Q

both delta H and S are neg.

A

spont. at low temps

43
Q

both delta H and S are pos.

A

spont. at high temps

44
Q

electrochemistry

A

study of relationships between electricity and chemical reactions

45
Q

oxidation numbers

A

used to track which element looses or gains e- during a rxn

46
Q

oxidation

A

loss of electrons, ox # increases

47
Q

reduction

A

gain of electrons, ox # decreases

48
Q

oxidizing agent

A

species which got reduced

49
Q

reducing agent

A

species that got oxidized

50
Q

for “in acidic soln”

A

do normal balancing procedure

51
Q

for “in basic soln”

A

do normal acidic soln procedure, then use OH- to balance out rxn

52
Q

voltaic (galvonic) cells

A

electrochemical cells w/ 2 half rxns separated into containers

53
Q

spont. redox rxn electron transfer

A

anode to cathode, energy is released

54
Q

anode

A

oxidation half rxn

55
Q

cathode

A

reduction half rxn

56
Q

salt bridge/ porous cup does what?

A

keeps the charges balanced

57
Q

do anodes loose or gain mass

A

loose

58
Q

do cathodes loose or gain mass

A

gain

59
Q

when loosing mass the concentration…

A

increases (vice versa)

60
Q

electrons from from — to —- potential energy

A

high to low

61
Q

electromotive force

A

potential difference between the anode and the cathode

62
Q

cell potential (Ecell)

A

-measured in volts (V)
- 1V = 1J/C

63
Q

higher reduction potential=

A

more likely to be reduced

64
Q

Ecell (naught)=

A

Ered (cathode)(naught) - Ered (anode)(naught)

65
Q

strongest oxidizing agents have most —— reduction potential

A

positive

66
Q

strongest reducing agents have most—– reduction potential

A

negative

67
Q

more positive E=

A

the cathode

68
Q

delta G (naught)= -n …

A

FE(naught)

69
Q

faraday’s constant, F =

A

96485 J/V mol

70
Q

spont rxn has a —— Ecell

A

positive

71
Q

concentration cell

A

galvonic cell prepared w/ same material for anode and cathode

72
Q

battery

A

portable, self contained electrochemical power source that consists of one or more voltaic cells, DC current

73
Q

primary cells

A

can only discharge once (non-rechargeable)

74
Q

secondary cells

A

rechargeable batteries, redox rxn can be reversed

75
Q

lead-acid battery

A

-for combustion engines
-reactants and products are solids
-made w/ lead and sulfuric acid

76
Q

Ni-Cd and Ni-metal hydride batteries

A

-lightweight, rechargeable
-hydrides replace Cd

77
Q

fuel cells

A

NOT BATTERIES, fuel is burned and converted to electricity (DC), source of energy must be continuously provided

78
Q

hydrogen fuel cells are ——–as efficient as combustion

A

twice

79
Q

corrosion

A

the oxidation which leads to structural and mechanical failure

80
Q

iron corrosion

A

rust

81
Q

copper corrosion

A

patina

82
Q

cathodic protection

A

introduce another metal which is easier to oxidize

GEN CHEM 2 (3 decks)

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