Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 2 > Chapter 18 Free Energy & Thermodynamics > Flashcards

Chapter 18 Free Energy & Thermodynamics Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Define Thermodynamics

A

Branch of physics concerned with heat and temperature and their relation to energy and work

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Define the 1st Law of Thermodynamics

A

Conversation of energy; energy can be transformed from one form to another, but can’t be created nor destroyed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

T/F According to the 1st Law of Thermodynamics energy is constant

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Define System

A

The material/process within which we are investigating the energy changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define Surroundings

A

Anything else that which the system can exchange energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is a good example of System and Surroundings?

A

Fire and balloon video, the balloon is the system receiving the impact of the fire, the room in which this is taking place is the surrounding, the area that can receive the exchange of energy occurring from the balloon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define State Function

A

Has a value that depends only on the state of the system, not how the system arrived at that state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Define the 2nd Law of Thermodynamics

A

States that over time, differences in temperature, pressure and chemical potential tend to disperse in a physical system that is isolated from the outside world

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Define Entropy

A

A measure of disorder in the system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

The Entropy of the universe is always _____________

A

Increasing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

In regards to Entropy, energy seems to go from _____________ to ______________

A

Concentrated; dispersed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define Spontaneous

A

A process that occurs without ongoing input of energy from outside the system (no force, it naturally occurs)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What are some examples of Spontaneous reactions?

A

I) Dissolution of NaCl in water

II) Melting of ice above zero degrees celsius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define Nonspontaneous

A

It is the very of Spontaneous reactions, due to the fact that it needs continuous input of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

A system going from an ordered state to a disorderly system has entropy that is _________ and is considered a _____________ reaction

A

Increasing; spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the equation used for Entropy?

A

ΔS = S final - S initial

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Spontaneous ΔS…

A

ΔS > 0 (positive value)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Nonspontaneous ΔS…

A

ΔS < 0 (negative value)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

At equilibrium ΔS…

A

ΔS = 0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

of microstate __________ means _______ disorderly and S __________

A

Increases; more; increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Predict the sign of ΔS for each process below
I) 2KClO3 (s) –> 2KCl (s) + 3O2 (g)
II) N2 (g) + 3H2 (g) –> 2NH3 (g)
III) 2O3 (g) –> 3O2 (g)

A

I) ΔS is positive b/c gas is generated
II) ΔS is negative b/c gas is reduced
III) ΔS is positive b/c gas is generated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

From solid to liquid to gas, Entropy ΔS __________

A

Increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the equation relating Entropy and system exchanging of heat

A

ΔS = Qrev / T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the process from a Gas to a Liquid phase?

A

Condensation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is the process from a Liquid to a Solid phase?

A

Freezing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is the process from a Solid to a Liquid phase?

A

Melting

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is the process from a Liquid to a Gas phase?

A

Vaporization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

T/F For any spontaneous process, the Entropy of the universe decreases

A

False; for any spontaneous process, the Entropy of the universe increases (ΔS > 0)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

ΔSuniverse = ΔS _______ + ΔS _________

A

System; surrounding

30
Q

Exothermic process __________ the Entropy of surroundings

A

Increases

31
Q

Endothermic process __________ the Entropy of surroundings

A

Decreases

32
Q

Change in Entropy of the surroundings is inversely proportional to what?

A

To the temperature at which the heat is transferred

33
Q

What is the equation relating Entropy of surrounding temperature dependence?

A

ΔS surrounding = -ΔHsystem / T

34
Q

Higher temperature (T), _______ change in Entropy of surrounding resulting in _______ ΔS surrounding

A

Less; smaller

35
Q

Lower temperature (T), _______ change in Entropy of surrounding resulting in _______ ΔS surrounding

A

More; larger

36
Q

Define Exothermic Relation to Entropy

A

Process that emits heat into the surroundings with (-ΔH system)

37
Q

Exothermic Relation __________ the entropy of the surroundings

A

Increases

38
Q

Equation showing Exothermic Relation to Entropy

A

ΔS = - (-Δ system) / T = +ΔS surrounding

39
Q

Define Endothermic Relation to Entropy

A

Process that absorbs heat from the surroundings with (+ ΔH system)

40
Q

Endothermic Relation __________ the entropy of the surroundings

A

Decreases

41
Q

Equation showing Endothermic Relation to Entropy

A

ΔS = - (+ΔH system) / T = - ΔS surrounding

42
Q

T/F The magnitude of the change in entropy of surroundings is not directly proportional to the magnitude of systems

A

False; the magnitude of the change in entropy of surroundings is proportional to the magnitude of systems

43
Q

Define Gibb’s Free Energy (G)

A

A thermodynamic state function related to Enthalpy (H) and Entropy (S)

44
Q

T/F Gibb’s Free Energy (G) is the minimum amount of work energy that can be released to the surroundings at constant T and P

A

False; Gibb’s Free Energy (G) is the MAXIMUM amount of work energy that can be released to the surroundings at constant T and P

45
Q

What can Gibb’s Free Energy (G) also be known as?

A

Chemical Potential

46
Q

What is the equation used for Gibb’s Free Energy (G)?

A

ΔG = ΔHsystem - TΔSsystem

47
Q

Spontaneous ΔG is…

A

ΔG < 0

48
Q

Nonspontaneous ΔG is…

A

ΔG > 0

49
Q

ΔG HAS to be __________ to be considered spontaneous

A

Negative

50
Q

ΔG ___________ when ΔH __________

A

Decreases; decreases

51
Q

ΔG ___________ when T ___________

A

Decreases; increases

52
Q

ΔG ___________ when ΔS __________

A

Decreases; increases

53
Q

ΔG is proportional to ______________

A

Negative Delta S universe

54
Q

To be spontaneous ΔG is _______ and ΔS universe is _______

A

ΔG < 0; ΔSuniverse > 0

55
Q

To be nonspontaneous ΔG is ______ and ΔSuniverse is _______

A

ΔG > 0; ΔSuniverse < 0

56
Q

If ΔH is negative and ΔS is positive what is the result of ΔG?

A

ΔG is negative meaning it is spontaneous at all temperatures

57
Q

If ΔH is positive and ΔS is negative what is the result of ΔG?

A

ΔG is positive meaning it is nonspontaneous at all temperatures

58
Q

If ΔH is negative and ΔS is negative what is the result of ΔG?

A

Since both ΔH and ΔS is negative ΔG’s value will be determined by the temperature

59
Q

When Delta H is negative and Delta S is negative what will Delta G be with regards to temperature?

A

Negative Delta G (spontaneous) with low temperature

Positive Delta G (nonspontaneous) with high temperature

60
Q

If ΔH is positive and ΔS is positive what is the result of ΔG?

A

Since both ΔH and ΔS is positive ΔG’s value will be determined by the temperature

61
Q

When ΔH is positive and ΔS is positive what will ΔG be with regards to temperature?

A

Negative ΔG (spontaneous) with high temperature

Positive ΔG (nonspontaneous) with low temperature

62
Q

Define the 3rd Law of Thermodynamics

A

Entropy of a perfect crystal at absolute zero (0 K) is zero

63
Q

How many ways can you arrange the components in a perfect crystal?

A

Only one possible way

64
Q

Define Standard Molar Entropy (S^o)

A

The entropy of one mole of the substance under standard state at 25 degrees celsius

65
Q

Entropy __________ when molar mass ___________

A

Increases; increases

66
Q

When is the only time you can apply and compare Entropy to molar mass values?

A

Only apply to elements in the same state (aka same column in the periodic table)

67
Q

Define Allotropes

A

Elements that can exist in 2 or more forms

68
Q

T/F Different arrangements of atoms leads to different standard molar entopies

A

True

69
Q

For a given state of matter, Entropy __________ when molecular complexity ___________

A

Increases; increases

70
Q

What is the equation used to show Entropy change for chemical reactions?

A

ΔS^o rxn =Σnp S^o (products) -Σnr S^o (reactants

71
Q

In the equation ΔS^o rxn =Σnp S^o (products) -Σnr S^o (reactants
What does p and r represent?

A

The stoichiometric coefficients of the products and reactants

72
Q

Define Standard Change of Free Energy for a Chemical Reaction

A

The change in free energy between the products and the reactants for a chemical reaction at standard states

Chemistry 2 (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions