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CHM 201 > CHM Exam 2 Flashcards (Chapter 9 and Chapter 10) > Flashcards

CHM Exam 2 Flashcards (Chapter 9 and Chapter 10)

1
Q

Energy

A

the capacity to do work or produce heat

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2
Q

First Law of Thermodynamics

A

energy is conserved and can be converted from one form to another

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3
Q

Energy is/isn’t a statement function

A

is

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4
Q

the internal energy for a system is the

A

sum of its potential and kinetic energy

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5
Q

the internal energy of a system can be changed by

A

work and heat

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6
Q

Internal energy formula

A

△E = q + w

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7
Q

work

A

force applied over a distance

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8
Q

Work is/isn’t a state function

A

isn’t

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9
Q

Heat

A

energy flow due to temperature difference

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10
Q

exothermic

A

energy as heat flows out of a system

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11
Q

endothermic

A

energy as heat flows into a system

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12
Q

Heat is/isn’t a state function

A

isn’t

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13
Q

Enthalpy forumla

A

H = E + PV

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14
Q

Formula for heat

A

q = mC△T

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15
Q

Enthalpy is/isn’t a state function

A

is

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16
Q

Hess’s Law

A

the change in enthalpy in going from a given set of reactants to a given set of products is the same whether the process takes place in one step or a series of steps

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17
Q

△H of reaction formula

A

△H(reaction) = sum of △H of products - sum of △H reactants

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18
Q

Heating an ideal gas at constant volume

A
  • no PV work done
  • all energy used to increase the translational energies of the gas molecules
  • bomb calorimeter
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19
Q

Heating an ideal gas at constant pressure

A
  • PV work done
  • energy is used to increase the translational energies of gas molecules and do work
  • coffee cup calorimeter
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20
Q

State function

A

refers to a property of a system that depends only on its present state

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21
Q

energy gained by the surroundings must be…

A

equal to the energy lost by the surroundings

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22
Q

work done by a gas

A

expansion

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23
Q

work done to a gas

A

compression

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24
Q

1 Latm = x J

A

101.325 J

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25
small font = flow = ?
work (w) and heat (q)
26
capital font = state function = ?
Energy (E) and Enthalpy (H)
27
q of system = ?
- q of surroundings
28
An open system can exchange ____ with its surroundings
energy and matter
29
A closed system can exchange ____ with its surroundings
only energy
30
A isolated system can exchange ____ with its surroundings
neither energy or matter
31
Water has a high heat capacity because
of its hydrogen bonds
32
exothermic = ? endothermic = ?
exothermic = negative endothermic = positive
33
formula for pressure
P = (w)/(-△V)
34
What are the 5 applications of thermochemistry?
1. phase changes 2. dissolution of solids into liquids 3. enthalpy of chemical reactions 4. redox chemistry 5. combustion of hydrocarbons
35
Energy in the universe is constant
1st law of thermodynamics
36
Second Law of Thermodynamics
states that for any spontaneous process there is always an increase with the entropy of the universe
37
Entropy
the thermodynamic function that describes the number of arrangements (positions and/or energy levels) available to a system existing in a given state
38
Nature spontaneously proceeds toward states that have the _____
highest probability of occurring
39
Using entropy, thermodynamics can ____
predict the direction in which a process will occur spontaneously
40
Entropy of universe formula
△S (universe) = △S (system) + △S (surroundings)
41
For a spontaneous process, △S (universe) must be
positive
42
△S (system) is dominated by
positional entropy
43
For a chemical reaction, △S (system) is dominated by changes in
the number of gas molecules
44
△S (surroundings) is determined by heat (formula?)
△S (surroundings) = (-△H)/(T)
45
△S (surroundings) is positive for exothermic processes because
△H is negative
46
Because △S (surroundings) depends inversely on T, exothermicity becomes more of an important driving force at
low temperature
47
Thermodynamics can/can't predict the rate at which a system will spontaneously change
can't
48
Third Law of Thermodynamics
states entropy of a perfect crystal at 0K is zero
49
Free energy is/isn't a state function
is
50
Free Energy
a process ocurring at constant temperature and pressure is spontaneous in the direction in which its free energy decreases
51
Standard state is at
25 C, and 1 atm
52
△G = 0
K = 1
53
△G < 0
K > 1, G products < G reactants
54
△G > 0
K < 1, G products > G reactants
55
positional microstates _____ as you go from a solid to a liquid to a gas
increase
56
Change in entropy formula
△S = nCln[T(final)/T(initial)]
57
Standard free energy change formula
△G = △H - T△S
58
the number of micro states ____ with the temperature _____
increases, increases
59
△G depends on _____ and _____
concentration and temperature
60
What are the three ways to find △G of a reaction?
1. △G = △H - T△S 2. △G = sum of △G(products) - sum of △G(reactants) 3. △G = -RTlnK
61
The thermodynamic quantity that expresses the degree of disorder in a system is
entropy
62
Which one is always positive when a spontaneous process occurs?
△S univ
63
What can be said about a chemical system that has reached a minimum in free energy?
The system has achieved equilibrium
64
A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if △H is _____ and △S is ______
+, +
65
For a reaction to be spontaneous under standard conditions at all temperatures, the signs of △H and △S must be _____ and ____ respectively
-, +T
66
The greater the dispersal of matter and/or energy in a system, the _____ the entropy
larger
67
The entropy of a substance always _____ as it changes from solid to liquid to gas
increases
68
When a pure solid or liquid dissolves in a solvent, the entropy of the substance _______
increases
69
When a gas molecule escapes from a solvent, the entropy _____
increases
70
Entropy generally increases with ______ molecular complexity since there are more moving electrons
increasing
71
Reactions increasing the number of moles of particles often ______ entropy
increase

CHM 201 (3 decks)

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