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Chem 152 > Quiz 3 > Flashcards

Quiz 3 Flashcards

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1
Q

Potential Energy

A

Energy an object has by virtue of its placement in a field of force, like gravity

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2
Q

PE = ?

A

mgh

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3
Q

Kinetic Energy

A

Energy an object has by virtue of its motion

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4
Q

KE = ?

A

1/2mu^2 and 3/2RT

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5
Q

When KE is at max, PE is at _____

A

minimum

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6
Q

When PE is at max, KE is at _____

A

minimum

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7
Q

Internal (total) energy =

A

KE + PE

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8
Q

Types of molecular kinetic energy

A

Translation, rotation, vibration

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9
Q

Translation

A

Motion through space

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10
Q

Rotation

A

Motion about the center of mass

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11
Q

Vibration

A

Motion directed through chemical bonds

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12
Q

In a molecule, where is PE stored?

A

Bonds

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13
Q

Electrostatic

A

Intermolecular attractions - molecule interacts with neighboring molecules

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14
Q

Thermodynamics

A

Study of energy and its interconversion

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15
Q

How can energy be transferred?

A

As heat or work

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16
Q

Heat (q)

A

Net transfer of energy between objects due to temp gradient

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17
Q

Work (w)

A

Force (energy) acting over a change in h/d to move an object

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18
Q

ΔE =

A

q+w

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19
Q

What does E describe?

A

The state of the system

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20
Q

When does the state of a chemical system change?

A

When the system exchanges energy as heat or work

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21
Q

Surroundings

A

Everything around the system

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22
Q

First law of thermodynamics

A

The total energy of the universe is constant

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23
Q

What direction does energy flow?

A

High E concentration to low E concentration

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24
Q

Exothermic Process

A

Evolution of system that results in heat transfer to surroundings q<0 (heat lost)

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25
Q

Endothermic Process

A

Evolution of system that results in heat transfer to system q>0 (heat gained)

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26
Q

Expansion

A

Vf > Vi and ΔV > 0 and w < 0

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27
Q

Compression

A

Vf < Vi and ΔV < 0 and w > 0

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28
Q

Work done on system by surroundings =

A

+w

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29
Q

Work done on surroundings by system =

A

-w

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30
Q

Heat/work in

A

+q and +w

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31
Q

Heat/work out

A

-q and -w

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32
Q

Pressure-volume work (PV)

A

Expansion of a gas against a constant external pressure

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33
Q

State functions/variables

A

Describe the momentary condition of thermodynamic system or difference between two momentary conditions

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34
Q

Examples of state functions/variables

A

E, ΔE, T, P, V, n, KE, PE

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35
Q

Process/path funcitons

A

Describe the energy change associated with a particular process imposed on a thermodynamic system

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36
Q

Examples of process/path functions

A

q and w

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37
Q

Do state function depend on the path the system takes?

A

No

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38
Q

Increase in system temp =

A

Increase in system’s heat energy content

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39
Q

What happens if heat is added at constant volume?

A

T and P increase

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40
Q

Is there work when V is constant?

A

No

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41
Q

What is the heat flow measured under constant P conditions?

A

ΔH

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42
Q

Which R value do you use for molar heat capacity?

A

8.314

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43
Q

Molar heat capacity (ΔE) definition

A

Energy required to raise the temp of 1 mole of substance by 1K

44
Q

What happens if heat is added at constant pressure?

A

T and V increase

45
Q

What is the heat flow measured under constant V conditions?

A

ΔE

46
Q

Molar heat capacity (ΔH) defintion

A

Enthalpy required to raise the temp of 1 mole of substance by 1K

47
Q

Is work done at constant pressure?

A

Yes

48
Q

Molar heat capacity definition

A

Energy required to raise the temp of 1 mole of a substance by 1K

49
Q

How do we go from Cv to Cp?

A

Add 1R

50
Q

For a polyatomic ion, are Cv and Cp greater than or less than Cv and Cp for a monatomic ion?

A

Greater

51
Q

Is losing heat exothermic or endothermic

A

Exothermic

52
Q

Isochoric

A

Constat Volume

53
Q

Isobaric

A

Constant Pressure

54
Q

Isothermal

A

Constant Temperature

55
Q

When do we use the 101.3 J/L*atm conversion factor?

A

When going from L*atm to Joules

56
Q

Hess’s Law

A

Going from one set of reactants to one set of products, overall change in enthalpy is the same (doesn’t depend on number of steps)

57
Q

Can we measure absolute enthalpies

A

No

58
Q

Calculate thermodynamics for compounds

A

Pure substance its normal phase at P = 1atm

59
Q

Calculate thermodynamics for solutions

A

Concentration of 1M

60
Q

Calculate thermodynamics for elements

A

The most stable form of the element at P = 1atm

61
Q

What subscript is used for standard state

A

º

62
Q

Standard enthalpy of formation (ΔHfº)

A

Enthalpy change that accompanies the formation of one mole of a compound from its elements with all substances in their stand states at 25ºC

63
Q

Spontaneous Process

A

Will occur in a system left to itself; no action from the surroundings is necessary to drive the process

64
Q

Non-spontaneous Process

A

Requires action from the surroundings to occur

65
Q

Second Law of Thermodynamics

A

The entropy of the universe is always increasing

66
Q

Are processes that lead to an increase in the entropy of the universe spontaneous or non-spontaneous

A

Spontaneous

67
Q

Configuration

A

General arrangement of a system, which can be achieved by one or microstates

68
Q

Microstate

A

Specific arrangement of a system corresponding to a particular configuration

69
Q

Weight (omega)

A

Number of microstates associated with a given configuration

70
Q

Entropy

A

Change in the arrangement of energy in response to a heat flow at a given temp

71
Q

What does rev mean in qrev?

A

Reversible (q flows very slow)

72
Q

ΔS (universe) > 0

A

Spontaneous

73
Q

ΔS (universe) < 0

A

Spontaneous in opposite direction

74
Q

ΔS (universe) = 0

A

At equilibrium

75
Q

Third Law of Thermodynamics

A

The entropy of a perfect crystal at 0 K is 0

76
Q

Standard Molar Entropy (S°)

A

Entropy change associated with heating one mole of a substance from 0 K to 298 K at 1 atm

77
Q

Entropy in exothermic process

A

ΔS (surroundings) > 0

78
Q

Entropy in endothermic process

A

ΔS (surroundings) < 0

79
Q

Entropy from gas to liquid

A

ΔS (system) < 0, ΔH (system) < 0, ΔS (surroundings) > 0

80
Q

Entropy from liquid to gas

A

ΔS (system) > 0, ΔH (system) > 0, ΔS (surroundings) < 0

81
Q

Do gases contract or expand at low T?

A

Contract

82
Q

Do gases contract or expand at high T?

A

Expand

83
Q

ΔG<0

A

Spontaneous

84
Q

ΔG>0

A

Spontaneous in opposite direction

85
Q

ΔG=0

A

Equilibrium

86
Q

When does the spontaneity of a rxn change?

A

After/before equilibrium

87
Q

When are exothermic rxns with ΔS<0 spontaneous (-ΔH and -ΔS) ?

A

At low temps

88
Q

When are exothermic rxns with ΔS>0 spontaneous (-ΔH and +ΔS) ?

A

At all temps

89
Q

When are endothermic rxns with ΔS>0 spontaneous (+ΔH and +ΔS) ?

A

At high temps

90
Q

What controls spontaneity when Tactual > X

A

ΔS

91
Q

What is X?

A

Temp at which spontaneity changes

92
Q

What controls spontaneity when Tactual < X

A

ΔH

93
Q

Tactual = X

A

Equilibrium

94
Q

Spontaneity when -ΔS and -ΔH

A

At low temps

95
Q

Spontaneity when +ΔS and -ΔH

A

All temps

96
Q

Spontaneity when +ΔS and +ΔH

A

High temps

97
Q

Spontaneity when -ΔS and +ΔH

A

No temps (never spontaneous)

98
Q

Standard Free Energy Change (ΔG°rxn)

A

Free energy change when reactants and products are in their standard state

99
Q

Standard Free Energy of Formation (ΔG°f)

A

Free energy change that occurs in the formation of 1 mol of a substance in its standard state from elements in their standard state

100
Q

If temperature is -Kelvin, what does that mean about the spontaneity?

A

Rxn is spontaneous at all temps

101
Q

What is ΔG ?

A

Free energy change for rxns occurring at any temp or concentration

102
Q

Whatis ΔG° ?

A

Change in free energy for a rxn involving compounds in their standard states

103
Q

If ΔG° < 0 then _____

A

K > 1

104
Q

If ΔG° = 0 then _____

A

K = 1

105
Q

If ΔG° > 0 then _____

A

K < 1

Chem 152 (4 decks)

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