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Sophomore- Spring 2024- Mac > Test 3 + some final stuff - Chem 112- Summer > Flashcards

Test 3 + some final stuff - Chem 112- Summer Flashcards

1
Q

Ksp

A

solubility equilibrium/solubility product constant, for ionic compounts treated as insoluble typically. Since it is a salt –><– cation + anion, the salt is a solid and is not included in the equilibra

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2
Q

molar solubility

A

moles/L of a saturated solution (so its the x in an ICE table or the E)

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3
Q

solubility

A

number of grams of solute in 1L of saturated solution

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3
Q

when Q < Ksp

A

no precipitate

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4
Q

when Q > Ksp

A

precipitate

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5
Q

Q= Ksp

A

no precipitate

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6
Q

factors that affect solubility

A

common ion effect, pH, formation of complex ions

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7
Q

common ion effect

A

suppresses the ionization of an electrolyte when another electrolyte (that contains a common ion) is added

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8
Q

how does pH affect solubility

A

solubility increases as the pH decreases (i.e. if you add an acid, the solubility will increase and move forward)

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9
Q

thermodynamics

A

the science dealing with heat and the relationship with other forms of energy. thermodynamics can predit whether a process will occur (but it does NOT predict amount of time required for process)

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10
Q

spontaneous process

A

occurs without outside intervention under specific set of conditions

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11
Q

nonspontaneous

A

does not occur without outside intervention (CONTINUAL input of external energy)

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12
Q

first law of thermodynamics

A

any change in internal energy is due to either heat or work (this energy can be kinetic or potential)

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13
Q

change in U

A

change in U = q + w

U is change in internal energy. q is heat. w is work.

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14
Q

thermochemistry

A

the study of the heat absorbed or released during chemical and physical changes

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15
Q

what is work

A

force applied x distance traveled. work involves movement

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16
Q

enthalpy letter

A

H,, change in H

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17
Q

enthapy def

A

a thermodynamic quantity.

change in H= change in U + P(change in V)

but it is also change in H = q (aka heat)

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18
Q

exothermic processes tend to be what

A

spontaneous. BUT this is not guarenteed

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19
Q

Entropy letter

A

S,, change in S

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20
Q

entropy def

A

entropy is a state function. it is a thermodymanic quantity that measures the amount of disorder in a system. to predict spontainiety, both enthapy and entropy must be known.

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21
Q

boltzman’s def

A

measure of disorder. S=KlnW

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22
Q

as temp increases ENTROPY of a system does what

A

decreases

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23
Q

S of different states

A

S gas > S liquid > S solid

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24
Q

more microstates = what

A

higher entropy

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25
Q

K = what

A

boltzmann’s constant (1.38 x 10^-23 J/K)

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26
Q

W= what

A

microstates (number of diff arrangements)

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27
Q

probabulity distributiion of microstates

A

W=X^N

X= number of cells in a volume
N = number of molecules

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28
Q

change in entropy

A

change in S system= S final- S initial

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29
Q

standard entropy

A

absolute entropy at 1 atm

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30
Q

choose one:

S increases with (larger/ smaller) molar mass

A

larger. entropy increases with larger molar mass

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31
Q

S increases with (more/ less) molar complexity

A

more molar complexity

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32
Q

change in S universe

A

= change in S system + change in S surroundings

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33
Q

change in S universe > 0

A

spontaneous

34
Q

change in S universe < 0

A

nonspontaneous (spontaneous in reverse reaction)

35
Q

change in S universe = 0

A

equilibrium

36
Q

Second law of thermodynamics

A

change in S universe stuff

37
Q

third law of thermodymanics

A

entropy of a pure perfect crystal substance at 0K is equal to 0. at 0, molecular movement stops. only one way to arrange the molecules at this point. Cannot go lower than 0K

38
Q

change in S (in relation to other S)

A

change in S= S products- S reactants

39
Q

gibbs free energy (def and equation)

A

measure of available energy. change in entropy is directly porportional to enthaply of a system

change in S surrounding = (-change in H system)/T

40
Q

gibbs free energy more direct equation

A

change in G = change in H - T (change in S)

41
Q

change in G < 0

A

spontaneous in forward

42
Q

change in G > 0

A

non spontaneous in forward

43
Q

change in G = 0

A

equilibrium

44
Q

what is G

A

gibbs free energy (spontaniety)

45
Q

spontaneous reactions generally have what

A

change in H < 0
change in S > 0
change in G < 0

46
Q

for a reaction to be spontaneous in low temp

A

change in G > 0 for an endothermic raction
or
change in G < 0 for an exothermic reaction

47
Q

exothermic reaction means what for change in H

A

change in H > 0

48
Q

exothermic reaction means what for change in H

A

change in H < 0

49
Q

for a reaction to be spontaneous in high temp

A

change in G < 0 for endothermic and exothermic

50
Q

for a reaction to be nonspontaneous in high temp

A

change in G > 0 for endothermic and exothermic

51
Q

for a reaction to be nonspontaneous in low temp

A

change in G> 0 for endothermic
or
change in G< for exothermic

52
Q

to find temp at which spontaneity changes when G=0

A

T= change in H/change in S

53
Q

standard free energy symbol and def

A

symbol = change in G degrees
def= free energy change for a reaction when it occurs under standard state conditions

54
Q
A
55
Q

when K >1, change in G degrees is what

A

when K >1= -( change in G degrees)

55
Q

when K < 1, change in G degrees is what

A

when K >1= + ( change in G degrees)

56
Q

when Q < K, change in G degrees is what

A

negative

57
Q

when Q > K, change in G degrees is what

A

positive

57
Q

addative free energy change

A

change in G 3= change in G 1 + change in G2

58
Q

oxidation

A

loss of electrons

59
Q

reduction

A

gaining electrons

60
Q

reducing reaction

A

loss electrons

61
Q

oxidizing agent

A

gain electrons

62
Q

hydrogen has what oxidation number

A

+1

63
Q

oxygen has what oxidation number

A

-2

64
Q

balancing redox reaction steps (acidic)

A
  1. write half reactions
  2. balance half reactions
  3. balance O by adding H2O
  4. balance H by adding H+
  5. balance charge by adding electrons
  6. make electrons =
  7. add half reactions together
65
Q

balancing redox reactions (basic)

A

normal steps +
1. for H+ ions, add on OH- to BOTH sides
2. make additional cancellations of all ner H20 molecules

66
Q

what are galvanic (voltaic) cells

A

cells that use spontaneous redox reactions to produce electrical energy

67
Q

anode

A

negatively changed metal electrode responsible for oxidation (the oxidation side of reaction)

68
Q

cathode

A

positive changed metal electrode responsible for reduction (the reduction side of reaction)

69
Q

why does current flow and what direction (anode vs cathode)

A

flows from anode to cathode. does this because there is a difference in electrical potential energy

70
Q

Ecell

A

electrical potential/cell potential. measured by voltmeter

71
Q

cell notation

A

left side is anode, right is cathode

72
Q

E degrees=

A

E cathode - E anode (you will need to look these values up)

73
Q

E degrees > 0

A

spontaneous

74
Q

E degrees < 0

A

nonspontaneous

75
Q

redox is spontaneous if (3 things)

A
  1. E degree cell is positive
  2. change in G degree is negative
  3. K is greater than 1
76
Q

if E degree is negative, it means what

A

non spontaneous, so charge is flowing from cathod to anode (reverse direction)

77
Q

when Q>1, E (< / >) E degrees

A

Q >1, E < E degrees

78
Q

when Q< 1, E (< / >) E degrees

A

Q< 1, E > E degrees

79
Q

when given numbers, which is the anode and which is cathode

A

the smaller one is anode, the larger is cathode

80
Q

for standard cell potential (the change in E degrees) equation, do you need to pay attention to stoichiometry?

A

no. so DON’T multiply to make them equal.

Sophomore- Spring 2024- Mac (11 decks)

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