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CH186—General Chemistry II > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

system

A

anything we define it as

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2
Q

open system

A

energy & mass can enter & exit

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3
Q

closed system

A

only energy can enter & exit; matter cannot

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4
Q

isolated system

A

neither energy nor mass can enter or exit

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5
Q

Surroundings

A

everything outside a defined system

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6
Q

state of a system

A

measurement of relevant properties (state functions)

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7
Q

state functions depend on…

A

final & initial states, not how they are achieved

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8
Q

9 state functions

A

mass

pressure

temperature

volume

particle number

entropy

enthalpy

Gibbs free energy

internal energy

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9
Q

heat

A

transfer of thermal energy between 2 bodies of different temp

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10
Q

q

A

heat

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11
Q

m

A

mass

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12
Q

P

A

pressure

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13
Q

T

A

temperature

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14
Q

B/V

A

volume

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15
Q

E

A

energy

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16
Q

U/I

A

internal energy

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17
Q

G

A

Gibbs free energy

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18
Q

H

A

enthalpy

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19
Q

S

A

entropy

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20
Q

entropy

A

measure of disorder

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21
Q

relation between entropy & moleculer weight

A

entropy rises & falls with molecular weight

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22
Q

EQUATION

S = _____ W

W =

Used for simple systems

A

S = K ln W

W = Xn

Xn = (cells in a volume)molecules

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23
Q

K = ___ + C

A

273

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24
Q

spontaneous or non-spontaneous:

(+/-) change in entropy

A

(+) = spontaneous

(-) = nonspontaneous

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25
Q

spontaneous or non-spontaneous:

(+/-) change in Gibbs

A

(+) = nonspontaneous when forward

(-) = spontaneous when forward

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26
Q

what is prime ‘ used for

A

living systems

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27
Q

K = Boltzman constant =

A

1.38 x 10-23

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28
Q

R = gas constant =

A

8.314 J/mol K

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29
Q

W =

A

number of different arrangements

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30
Q

Xn =

A

(cells in a volume)molecules

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31
Q

Avogadro’s number

A

6.022 x 1023

32
Q

standard conditions

A

1 atm

1.00 M

pH 7

25 C

pure solids & liquids

most stable allotropic form of elements at std conditions

33
Q

1st law of TD

A

energy cannot be created or destroyed, only transduced

34
Q

2nd law of TD

A

entropy of the universe is always increasing

35
Q

3rd law of TD

A

the entropy of a perfect crystalline substance is zero at 0 K

36
Q

spontaneous process

A

occurs under a specific set of conditions

37
Q

S increases with… (5)

A

molar mass

molecular complexity

temperature

volume

when a rxn produces more gas molecules than it consumes

38
Q

exergonic

A

products at lower energy state than reactants

G is (-)

39
Q

endergonic

A

products at higher energy state than reactants

G is (+)

40
Q

When H is (-) and S is (+), G is ___ and will be _______

A

negative

spontaneous

41
Q

When H is (+) and S is (-), G is ___ and will be __________

A

positive

non-spontaneous

42
Q

2 necessary components of an effective collision

A
  • enough Ea
  • correct orientation
43
Q

there are more effective collisions with…

A

increased temp, stirring, increased concentration

44
Q

reaction rate is proportional to…

A

effective collisions per second

45
Q

activation energy

A

minimum energy required to initiate reaction

46
Q

effective collisions result in…

A

an activated complex during the transition state

47
Q

average rate

A

change in concentration over a specific period of time

48
Q

instantaneous rate

A

rate of the reaction at one point in time

49
Q

instantaneous rate =

A

k[A]

k = rate constant

50
Q

RATE EXPRESSION

A
51
Q

rate law definition

A

equation that relates the rate of reaction to the concentration of reactants

52
Q

rate law (in general)

A

rate = k[A]x[B]y

53
Q

x in rate law =

A

order of A

54
Q

y in rate law =

A

order of B

55
Q

To find X & Y in rate law

A
  • in the information given, find 2 different concentrations of A in which the concentration of B is constant
  • divide one by the other
  • for these same sets of data, divide one rate of A by the other rate of A
  • rate quotient = (concentration quotient)x or y
  • do the same for B, using y
56
Q

find the exponent in TI-83

A

log(product) / log(base) = exponent

57
Q

how to do inverse of natural log

A

ln(x) = y

→

x = ey

58
Q

A in Arrhenius equation =

A

collision frequency/frequency factor

59
Q

how to find overall reaction order

A

sum of the exponents on reactants in rate law

60
Q

3 important things about rate law

A
  • exponents must be determined from experimental data
  • rate depends on concentration of reactants
  • reaction order is determined by reactant concentrations, never product concentrations
61
Q

intermediates

A

species that appear in reaction mechanism, but not products or reactants

62
Q

elementary reaction

A

single collision of reactant molecules

63
Q

molecularity

A

number of reactant molecules involved in a collision

64
Q

unimolecular, bimolecular, termolecular

A

refers to # of reactant molecules in an elementary reaction

65
Q

rate-determining step

A

slowest step in reaction

66
Q

2 requirements for reaction mechanisms

A
  • sum of elementary reactions must be the balanced overall equation
  • rate-determining step must have the same rate law as that determined by experimental data for the overall reaction
67
Q

step with the highest Ea

A

rate-determining step

68
Q

catalyst

A

substance that increases rate of reaction by providing an alternate pathway for the reaction with a lower Ea

69
Q

catalysts reduce…

A

entropy

importance of colliding at correct orientation

70
Q

heterogeneous catalyst

A

reactants & catalysts in different phases

71
Q

homogeneous catalyst

A

reactants & catalysts in the same phase

72
Q

homogenous catalysts are often ______ and can be used at ______

A

acids

1 atm

73
Q

enzymes

A

biological catalysts

74
Q

enzymes use…

(r/t TD)

A

coupling

75
Q

causes catalysis to plateau

A

saturation

CH186—General Chemistry II (6 decks)

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