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Chem 1B > thermo > Flashcards

thermo Flashcards

1
Q

What is a spontaneous process

A

a process that occurs without outside intervention

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2
Q

What is true about chemical systems

A

they want to be at the lowest chemical energy

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3
Q

What is Gibbs free energy

A

it is a thermodynamic state function where chemical systems tend towards the lowest chemical potential also called Gibbs Free Energy

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4
Q

Why is Gibbs free energy called the chemical potential

A

it determines the direction of chemical systems

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5
Q

what corresponds to a spontaneous process

A

a decrease (negative) in ∆G

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6
Q

what corresponds to a nonspontaneous process

A

an increase (positive) ∆G

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7
Q

When is ∆G at equilibrium?

A

When it equals zero, that is the lowest chemical potential

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8
Q

How is ∆G calculated?

A

Gfinal-Ginitial

or ∆H-T∆S

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9
Q

When is the change in enthalpy exothermic?

A

When ∆H is negative (energy/heat is released)

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10
Q

When is the change in enthalpy endothermic?

A

When ∆H is positive (energy/heat is absorbed)

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11
Q

What is Entropy (∆S)

A

It is the number of energetically equivalent ways to arrange a component of a system

when there are more ways to arrange the particles, the particles are more randomized in the chemical system (increase in Entropy)

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12
Q

When ∆S is positive

A

The entropy has increased

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13
Q

What are the four changes that increase entropy

A

Phase change

Increases in temperature

Reactions where there are a larger # of product molecules than reactant molecules

Solids dissociating in water

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14
Q

How does ∆G relate to temperature?

A

It is temperature dependent based on the context

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15
Q

In the equation ∆G=∆H-T∆S, what are the two cases when ∆G is temperature dependent?

A

When ∆H = (+) and ∆S=(+)

When ∆H=(-) and ∆S=(-)

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16
Q

When is ∆G nonspontaneous at all temperatures?

A

When ∆H = (+) and ∆S= (-)

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17
Q

When is ∆G spontaneous at all temperatures

A

When ∆H=(-), ∆S=(+)

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18
Q

When are the standard conditions?

A

For solutions, the concentrations are @ 1M

For gas, the pressure is = 1 atm

For temp, 25C and 298K is the most stable temperature

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19
Q

When is the ∆Gf of an element = to zero?

A

When it is in its elemental state

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20
Q

What affects the standard molar entropy?

A

A particle in its gaseous state has a higher entropy since it has more ways to arrange its particles

When an atom increases its size (down a column) it has more space for energy to disperse

More complex molecules (more atoms) have more ways to arrange those atoms and have more ways to disperse eneergy

Dissolution of a solid to liquid allows for more ways to arrange particles

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21
Q

When we lose moles in a reaction, what happens to the entropy?

A

The entropy decreases

22
Q

How to find Gibbs Free Energy under non-standard conditions

A

∆G=∆G°+RTlnQ

23
Q

What does it mean when ∆G° is negative

A

It is spontaneous in the forward direction, it is product favored K>1

24
Q

What does it mean when ∆G° is positive

A

It is nonspontaneous in the forward direction, it is reactant-favored K<1

25
Q

When ∆G is negative what does it mean in relation to spontaneity and K

A

it is spontaneous in the forward direction and is product favored

K>1

26
Q

When ∆G is positive, what does it mean in relation to spontaneity and K

A

it is nonspontaneous in the forward direction and is reactant favored

K<1

27
Q

What is an oxidation-reduction reaction

A

the transfer of electrons from one substance to another

28
Q

what is oxidation

A

the loss of electrons

29
Q

what is reduction

A

the gain of electrons

30
Q

What does it mean to be the reducing agent

A

it is the substance that is oxidized and it loses the electrons so that the other substance gains them

31
Q

what does it mean to be the oxidizing agent

A

it is the substance that is reduced, it gains the electrons that the oxidized element loses

32
Q

what is the electrical current

A

it is the flow of electrons driven by the difference in potential energy

33
Q

what is a voltaic cell

A

it is a electrochemical cell that produces an electrical current from a spontaneous redox reaction

34
Q

What happens at the anode?

A

it is the site of oxidation, it is where electrons are produced to flow to the cathode

it has a higher potential energy since it has more electrons

35
Q

what happens at the cathode

A

it is the site of reduction, it has a lower potential energy so electrons flow here

36
Q

How do electrons move from anode to cathode

A

they move spontaneously by the change in potential energy between the anode and the cathode

37
Q

When E°Cell is positive

A

the reaction is spontaneous

38
Q

When E°cell is negative

A

the reaction is nonspontaneous

39
Q

What is E° Cell

A

The chemical potential at standard conditions

40
Q

what is E cell

A

the chemical potential at non-standard conditions

41
Q

what is SHE

A

it is the standard hydrogen electrode that has a potential of 0.00 V

42
Q

On the Reduction Half-Reaction table, what is the left hand side?

A

the oxidizing agents (they are reduced (consume electrons))

43
Q

What is the right hand side of the Reduction Half-Reaction table?

A

they are reducing agents (they are oxidized)

44
Q

What does it mean that F has the highest placement on the Reduction Half Reaction table?

A

it is the best- oxidizing agent

45
Q

what does it mean to be higher up (more positive) on the reduction half-reaction table?

A

it favors reduction

46
Q

what does it mean to be lower (more negative) on the reduction half-reaction table?

A

it favors oxidation (the back reaction)

47
Q

Reactions on the higher end of the table tend to be better ______ agents

while reactions on the lower end of the table tend to be better _______ agents

A

oxidizing agents

reducing agents

48
Q

All half reactions are written as

A

reductions

49
Q

When E° is more positive on the table

A

it is reduction favored

(PIR)
positive is reduction

50
Q

When E° is more negative on the table

A

oxidation is favored

(NIO)
negative is oxidation

51
Q

In general what is true about oxidizing agents and reducing agents on the table and their placements above or below other reactions?

A

an oxidizing agent will oxidize any reducing agent below it

a reducing agent will reduce an oxidizing agent above it

52
Q
A

Chem 1B (7 decks)

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