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CHEM1212 > TEST 2- 17.1-17.7, 17.10, 11 > Flashcards

TEST 2- 17.1-17.7, 17.10, 11 Flashcards

1
Q

First law of thermodynamics

A

energy cannot be created or destroyed, only transferred

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2
Q

The internal energy of an isolated system

A

remains constant

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3
Q

The total energy of the universe is

A

constant, and change in energy of universe is 0

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4
Q

The first law of thermodynamics describes

A

organized energy

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5
Q

Second law of thermodynamics

A

all spontaneous energy transfers in the universe serve to increase overall entropy (s) of universe

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6
Q

Reversible process

A

does not increase entropy of universe, can be undone by reversing conditions, can be forward or reverse on path

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7
Q

Irreversible process

A

does increase the entropy, cannot be undone

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8
Q

Spontaneous reaction or change

A

continue to occur on its own without outside forces

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9
Q

Spontaneous reactions will result in

A

increase in disorder (entropy) of universe

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10
Q

Spontaneous processes do not need

A

continuous input of energy

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11
Q

Nonospontaneous process

A

does not occur in specific conditions and requires an input of energy

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12
Q

Organized energy of universe

A

goes down, disorganized energy goes. up

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13
Q

The second law of thermodynamics describes

A

disorganized energy

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14
Q

Third law of thermodynamics

A

as temp increases so does entropy, as temp decreases so does entropy

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15
Q

At 0 K

A

absolute 0, entropy is 0

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16
Q

Entropy

A

increase in randomness or dispersal of matter and energy in J/Kxmol

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17
Q

Standard entropy

A

absolute entropy at pressure 1 atm

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18
Q

Microstates

A

all the microscopic distributions of energy among particles in a system that are possible, while maintaining the macroscopic form

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19
Q

Entropy related to microstates equation

A

S = Kbln(W)

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20
Q

Kb

A

boltzman’s constant- 1.318 x 10^-23 J/K

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21
Q

W

A

number of microstates

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22
Q

A decrease in pressure or increase in volume

A

Increases entropy

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23
Q

A decrease in pressure means an increase in

A

volume, energy has more space to disperse

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24
Q

Larger molecule size allows for more

A

microstates and greater entropy

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25
Q

Two substances of the same substance in same state

A

larger sample will have more entropy

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26
Q

A process with an increase in the number of gas particles will result in

A

overall increase in entropy

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27
Q

Mixing substances will cause

A

increase in overall entropy, solid has higher entropy when dissolved than when in solid form

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28
Q

Two compounds with similar mass in same phase

A

more complex means a greater entropy

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29
Q

Enthalpy in exothermic processes

A

enthalpy is negative, system releases energy, heat of surroundings is greater than 0, heat of system is less than 0, and ENTROPY of surroundings is greater than 0

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30
Q

Enthalpy in endothermic process

A

enthalpy is positive, system absorbs energy, heat of system is greater than 0, heat of surroundings is less than 0, and ENTROPY of surroundings is less than 0

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31
Q

Energy gained by the surroundings is equal to

A

the energy lost by the system, qsurroundings = - qsystem

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32
Q

Change in entropy of phase change =

A

change in enthalpy of change divided by temperature where change occured

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33
Q

Positive value of change in entropy

A

increase in entropy, favorable, spontaneous

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34
Q

Change in entropy of universe =

A

Change in entropy of system + change in entropy of surroundings, Change in entropy of system + enthalpy of surroundings / temp

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35
Q

Change in entropy surroundings =

A
  • Change in enthalpy system / Temp at constant pressure
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36
Q

How to find enthalpy and entropy change for chemical reactions

A

change in products - change in reactants

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37
Q

Free energy

A

state function that combines enthalpy and entropy

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38
Q

Gibbs free energy

A

usable energy, energy available to do work, Change in Gibbs energy = Change in enthalpy - Temperature (Change in entropy) (entropy of SYSTEM)

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39
Q

Exergonic reactions

A

negative free energy, lose usable energy as the process moves forward, spontaneous in forward direction, nonspontaneous in the reverse

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40
Q

Endergonic reactions

A

positive free energy, gain usable energy, nonspontaneous in the forward, spontaneous in the reerse

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41
Q

If gibbs free energy = 0

A

reaction is in equilibrium and no net change will occur

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42
Q

If Change in H is negative and Change in S is positive

A

reactions are spontaneous at all temperatures

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43
Q

If Change in H is negative and Change in S is negative

A

reactions are spontaneous at low temperatures

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44
Q

If Change in H is positive and Change in S is positive

A

reactions become spontaneous at high temperatures

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45
Q

If Change in H is positive and Change in S is negative

A

reactions are non-spontaneous at all temperatures

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46
Q

Solute

A

substance that experiences a phase change after dissolved

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47
Q

Solvent

A

the media that remains in that same phase after a solution is formed, solute is dissolved in this

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48
Q

Molarity and temperature

A

temperature dependent

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49
Q

The sum of mole fractions

A

always equals 1

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50
Q

Mole fraction and temperature

A

temperature independent

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51
Q

Mole fraction

A

Number of moles of A / number of moles of A + B

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52
Q

Molality

A

m, moles of solute / kg of solvent

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53
Q

Molality and temperature

A

temperature independent

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54
Q

Mass percent

A

Mass of component / total mass of components x 100

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55
Q

Mass percent and temperature

A

temperature independent

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56
Q

Parts per million

A

mass of solute / mass of solution x 10^6

57
Q

Parts per billion

A

mass of solute / mass of solution x 10^9

58
Q

Parts per million simplified equation

A

mg solute / kg solution

59
Q

Parts per billion simplified equation

A

ug solute / kg solution

60
Q

Unsaturated solution

A

solute’s concentration is lower than its solubility

61
Q

Saturated solution

A

solute’s concentration is equal to its solubility

62
Q

Supersaturated solution

A

solute’s concentration is greater than is solubility

63
Q

Miscibility

A

ability of one liquid to dissolve in another liquid

64
Q

Miscible

A

liquids successfully mix

65
Q

Immiscible

A

liquids. do not mix

66
Q

Two liquids are miscible phrase

A

like dissolves like

67
Q

For a solution to form spontaneously

A

there is an exothermic change in the system (decrease in internal energy), increase in entropy (increase in disorder)

68
Q

An increase in entropy ALWAYS occurs when

A

a solution has been made

69
Q

Solutions being combined

A

is more energetically favorable that liquids on their own

70
Q

Solute molecules need to

A

separate and spread out from other solute molecules

71
Q

Solute molecules separating is a __ process

A

endothermic

72
Q

Solvent molecules need to

A

separate and spread out from other solvent molecules

73
Q

Solvent molecules separating is a __ process

A

endothermic

74
Q

Solute molecules interacting directly with solvent molecules is a __ process

A

exothermic

75
Q

Direction formation of a solution is a __ process

A

exothermic

76
Q

If more energy was required to break bonds in solute and solvent than energy released in solution formation

A

overall heat of solution is endothermic

77
Q

If the heat of solution is positive (endothermic)

A

adding heat will increase solubility of the solute

78
Q

If more energy was released in the solution formation than energy required to break the bonds in the solute and solvent

A

overall heat of solution is exothermic

79
Q

If the heat of solution is negative (exothermic)

A

adding heat will decrease solubility of the solute

80
Q

As atomic radius of an ion decreases

A

the heat of hydration is more exothermic

81
Q

As atomic radius of an ion increases

A

the heat of hydration is more endothermic

82
Q

As the charge of two ions of similar size increases

A

(same period), the heat of hydration is more exothermic

83
Q

As hydration processes become more exothermic

A

the process is becoming more spontaneous

84
Q

Henry’s law

A

solubility of a gas in a solution is directly proportional to the partial pressure of the gas

85
Q

As pressure increases, solubility of gas

A

will also increase

86
Q

As volume increases, solubility of gas

A

decreases

87
Q

As temperature increases, solubility of gas

A

decreases

88
Q

Van’t Hoff Factor

A

moles of particles in solution / moles of solute dissolved

89
Q

Experimentally determined VHF will always be

A

lower than the ideal

90
Q

Percent ionization formula

A

= (experimental VHF -1) / (ideal VHF -1) x 100

91
Q

Colligative properties depend on

A

the number of particles of solute and solvent and not the identity of the solute

92
Q

Adding solute to a liquid has the effect of

A

lowering the vapor pressure

93
Q

Raoult’s law

A

how the vapor pressure of liquid changes as a solute is added to the liquid

94
Q

Raoult’s law formula

A

Vapor pressure of solution = mole fraction of solvent x vapor pressure of pure solvent

95
Q

If we create a liquid-liquid system where both components are volatile

A

Ptotal = X solv 1 x Vapor pressure solv 1 + X solv 2 x Vapor pressure solv 2

96
Q

Boiling point elevaiton

A

solute dissolved in liquid, solute lowers vapor pressure of liquid and boiling point increases

97
Q

Boiling point elevation equation

A

Change in Tb = Kb(m)(I)

98
Q

Freezing point depression

A

solute dissolved in liquid, solute interrupts ability of liquid to interact which decreases freezing point

99
Q

Freezing point increases when molality

A

decreases

100
Q

When solute increases, vapor pressure and boiling point

A

vapor pressure decreases, boiling point increases

101
Q

Osmotic pressure

A

amount of pressure required to prevent the flow of a pure solvent into a solution through semi-permeable membrane

102
Q

Osmotic pressure equation (pi)

A

pi = nRT / V (I)

103
Q

R gas constant for osmotic pressure

A

R = 0.0821 L x atm / mol

104
Q

Osmosis

A

movement of water from low concentration of solute to high

105
Q

In osmosis solute cannot

A

move across semi-permeable membrane

106
Q

Entropy increases with __ IMF

A

decreasing

107
Q

Microstates increase with __ temperature

A

increasing

108
Q

Temperature increases with __ entropy

A

increasing

109
Q

Forming bonds

A

releases energy

110
Q

Formation of solution steps

A

break solute-solute (exo), break solvent-solvent (exo), form solute-solvent (endo)

111
Q

Favor spontaneous reactions

A

decrease in internal energy, increase in disorder

112
Q

Ion-dipole attraction

A

electrostatic, between ion and molecule with a dipole, H2O molecules surround and solvate the separated ions, physical process, dissociation

113
Q

If ion-dipole attraction dominate

A

compound it pulled in solution is highly soluble

114
Q

If force of attraction between oppositely charged ions is dominate

A

component is undissolved in solid state, low water solubility

115
Q

Solubility

A

rate is dissolution is equal to rate of precipitation

116
Q

Supersaturated

A

concentration is greater than solubility

117
Q

Unsaturated

A

concentration is lower than solubility

118
Q

Exothermic temperature decreases and solubility

A

increases

119
Q

Endothermic temperature increases and solubility

A

increases

120
Q

Ionic and covalent solids

A

can dissolve

121
Q

Solid dissolving in a liquid

A

endothermic

122
Q

Solubility of solids __ with increasing temperature

A

increases

123
Q

Increasing heat favors

A

formation of products

124
Q

Miscible

A

two liquids that mix in all properties (ethanol, water)

125
Q

Immiscible

A

two liquids that do not mix to an extent, NP liquids, gases, hydrocarbonds, water

126
Q

Partially miscible

A

two liquids that are moderately soluble, bromine, water

127
Q

Dissolution of gas in liquid

A

exothermic

128
Q

Gas solubility decreases

A

temperature increases

129
Q

Gas solubility and partial pressure

A

directly proportional

130
Q

Making supersaturated solutions

A

high temperature, slowly cool, solid wont precipitate, at low temp solute concentration is greater than compound solubility

131
Q

Molality

A

moles solute / kg solvent

132
Q

More solute = ___ vapor pressure

A

decreasing

133
Q

Solution boils at higher or lower temperature than pure solvent

A

higher

134
Q

Boiling point elevation and freezing point depression are direct results of

A

vapor pressure lowering

135
Q

Saturated solutions are

A

at equilibrium

136
Q

Water evaporated unsaturated solution, vapor pressure above solution

A

decreases

137
Q

Water evaporated saturated solution, vapor pressure above solution

A

equal

138
Q

Intensive properties

A

units of concentration do not depend on size or amount

CHEM1212 (5 decks)

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