Chapter 17 Flashcards

1
Q

What is the driving force for a spontaneous process?

A

Increase in entropy of the universe

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2
Q

In any spontaneous process there is always?

A

An increase in entropy of the universe

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3
Q

Entropy changes in the surroundings are primarily determined by?

A

heat flow

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4
Q

the impact of heat transferring from the surroundings will be greater at?

A

lower temperatures

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5
Q

A process at constant temperature and pressure is spontaneous only when?

A

ΔG is negative

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6
Q

When a reaction involves gaseous molecules, the change in positional entropy is dominated by?

A

the number of molecules of products and reactants.

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7
Q

gaseous products > gaseous reactants.

positional entropy______
ΔS is _______

A

positional entropy increases
ΔS is positive

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8
Q

gaseous products < gaseous reactants.

positional entropy______
ΔS is _______

A

positional entropy decreases
ΔS is negative

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9
Q

the equilibrium position represents what?

A

the lowest free energy value available to a reaction system.

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10
Q

The maximum amount of useful work is equal to?

A

ΔG (change in free energy)

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11
Q

Achieving maximum work can only be achieved via hypothetical pathway because?

A

Any real pathways waste energy.

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12
Q

In any real cyclic process (beginning and end have same result) in the system work is changed to what and where?

A

heat in the surroundings

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13
Q

In any real cyclic process in the system, the entropy of the universe?

A

increases

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14
Q

As we use energy what happens?

A

we degrade its usefulness

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15
Q

What does 1st law of thermodynamic not tell us?

A

Why something happens in the direction it does

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16
Q

in thermodynamics entropy tells us?

A

the # of arrangements or micro states in a system

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17
Q

positional entropy

A

the probability of a particular state depending on number of ways arrangement can be obtained

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18
Q

the entropy of the universe is increasing but energy is?

A

constant

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19
Q

for anything to be spontaneous the entropy of the universe must be?

A

positive

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20
Q

ΔS universe +
Entropy _____
Process is _____

A

increasing
spontaneous

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21
Q

ΔS universe -
Entropy ______
Process is _____

A

decreasing
non-spontaneous in desired direction

22
Q

ΔS is 0

A

equilibrium is reached

23
Q

Magnitude of ΔS surroundings is dependent on?

A

temperature

24
Q

Exothermic
ΔS surr _____
ΔS universe ____

25
Endothermic ΔS surr _____ ΔS universe ____
- +
26
ΔH - TΔS + ΔG?
- (spontaneous)
27
ΔH? TΔS + ΔG -
-
28
ΔH - TΔS? ΔG -
+
28
ΔH- TΔS - ΔG?
spontaneous if ΔH is greater than TΔS (low temperature)
29
ΔH + TΔS + ΔG?
spontaneous if TΔS is greater than ΔH (high temperature)
30
ΔH + TΔS - ΔG?
+ (non- spontaneous)
31
Third law of thermodynamics
The entropy of a perfect crystal at 0K is zero
32
What is the main idea behind the third law of thermodynamics?
there is absolute order/ no disorder since everything is in perfect position.
33
the more negative ΔG value,what direction does the reaction shift?
to the right to achieve equilibrium
34
Entropy depends on what?
volume and pressure
35
K= 1
equilibrium
36
K<1,where does reaction shift?
shift to left
37
K >1
shift to right
38
if shifting to the left it is _____ favored?
reactant
39
If shifting to the right it is ______ favored?
product
40
Equilibrium is not always ____ for thermodynamics?
half & half
41
If ΔG is zero it means?
free energy of products and reactants are equal
42
ΔG < 0, then k is?
>1
43
ΔG > 0, then k is?
<1
44
if k is 1 then pressure is?
1 atm
45
If ΔG is <0, it meanswhat about standard energy?
standard energy of the products is less than the standard energy of the reactants
46
Since products has less free energy the shift must be?
right (product favored)
47
ΔG < 0 product pressure _____ reactant pressure ____
greater than 1atm less than 1 atm
48
If reactants have lower free energy, then shift must be?
left (reactant favored)
49
equilibrium shifts from?
high energy to low energy
50
ΔG > 0 reactant pressure _____ product pressure ______
> 1 atm < 1 atm
51
Free energy
energy available to do work