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Chemistry Lecture > Exam Four > Flashcards

Exam Four Flashcards

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1
Q

A large K value means a […] value of G.

A

large

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2
Q

Equation of delta G:

A

DG = -(RTlnK)

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3
Q

When K > Q, the reaction proceeds […] and the reaction is […].

A

towards the products; spontaneous

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4
Q

When K < Q then the reactions proceeds […] and is […].

A

towards the reactants; nonspontaneous

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5
Q

S and T relationship:

A

entropy is directly related to the temperature (as T increases so does S)

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6
Q

What causes an increase in entropy?

A
  1. increase in temperature

2. s < l < aq

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7
Q

Calculating the entropy of the universe steps:

A
  1. CALCULATE DH: [Heats of formation (P-R)]
  2. CALCULATE SURROUNDINGS: (-DH/T)
  3. CALCULATE UNIVERSE: (Ssys + Ssurr)
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8
Q

At equilibrium DSuniverse =

A

0; so DSsys = -DSsurr

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9
Q

Can a reaction occur spontaneously even though DSsys is negative?

A

yes; if the DH is negative (DSsurr will be positive)

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10
Q

Can a reaction occur spontaneously when the reaction is endothermic?

A

yes; only if DSsys > DSsurr

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11
Q

Predict:

DH = -
DS = +
A 
spontaneous at all T
DG is (-)
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12
Q

Predict:
DH = +
DS = -

A

nonspontaneous at all T

DG = (+)

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13
Q

Predict:
DH = +
DS = +

A

spontaneous at higher T; nonspontaneous at lower T

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14
Q

Predict:
DH = -
DS = -

A

spontaneous at lower T; nonspontaneous at higher T

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15
Q

What is the equation to solve the temperature at which a reaction becomes spontaneous:

A

DH = T(DS) and T = (DH)/(DS)

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16
Q

How do you balance a redox reaction in an acidic medium?

A
  1. separate into half-reactions and determine which is being oxidized/reduced
  2. first balance all atoms other than O and H
  3. balance O molecules by adding H2O
  4. balance H by adding H+ ions
  5. balance charge by adding electrons (multiply if needed so electrons equal)
  6. add the half reactions
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17
Q

How do you balance a redox reaction in a basic medium?

A
  1. separate into half-reactions and determine which is being oxidized/reduced
  2. first balance all atoms other than O and H
  3. balance O molecules by adding H2O
  4. balance H by adding H+ ions
  5. balance charge by adding electrons (multiply if needed so electrons equal)
  6. balance H+ ions by adding OH- ions to both sides of the reaction (formation of H2O)
  7. add the half-reactions
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18
Q

If the salt is pure, predicting the products of its electrolysis is straightforward…

A

the cation will be reduced and the anion oxidized

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19
Q

The more easily reduced agent species is the stronger […] agent.

A

oxidizing

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20
Q

The more easily oxidized species is the stronger […] agent.

A

reducing

21
Q

How do you determine the relative strengths of electrode species molten salts?

A

NOT cell potential; use periodic trends

22
Q

ELECTROLYSIS:
If the metal holds its electrons more tightly it has a […]. Thus, as a […] , it gains electrons more easily, so it is the stronger […] agent and is […] at the cathode.

A

higher ionization energy; cation; oxidizing agent; reduced

23
Q

ELECTROLYSIS: If the nonmetal holds its electrons less tightly than another, it has a lower […]. Thus, as […]. it loses electrons more easily, so it is the stronger […] agent and it is […] at the anode.

A

electronegativity (EN); an anion; reducing; oxidized

24
Q

ELECTROLYSIS: How do you predict the electrode products of aqueous salt solutions?

A
  1. reduction with the less negative (more positive) electrode
  2. oxidation with the less positive (more negative) electrode potential occurs
25
Q

Cations of less active metals are […] to the metal.

A

reduced

26
Q

List less active metals:

A

Au, Ag, Cu, Cr, Pt, Cd

27
Q

Cations of more active metals are […] to the metal.

A

not reduced

28
Q

List active metals:

A

Group 1A, 2A, and Al

29
Q

Anions that are […] because of overvoltage from O2 formation include […] except […].

A

oxidized; halides; F-

30
Q

Anions that are not oxidized include…

A

F-

common oxoanions (SO4, CO3, NO3, PO4)

31
Q

Voltaic cells are also known as…

A

galvanic cells

32
Q

A voltaic cell uses a […] redox reactions to generate electrical energy.

A

spontaneous

33
Q

List the characteristics of voltaic cells:

A
  1. spontaneous
  2. electrical energy generated from the difference in free energy between higher energy reactants and lower energy products
  3. system does work on the surroundings (load)
34
Q

List the characteristics of electrolytic cells:

A
  1. uses electrical energy to drive a nonspontaneous redox reactions
  2. external power source supplies free energy to convert lower energy reactants into higher energy products
  3. surroundings (power supply) do work on the system (electrolytic cell)
  4. electroplating and the recovery of metals from ores utilize this
35
Q

What is the notation for a volatic cell?

A
  1. anode on the left (X—X+)
  2. cathode on the right (Y+—Y)
  3. anode/cathode separated by physical boundary
  4. comma separates the half cell components that are in the same phase
  5. concentrations are placed in parathesis
36
Q

The more positive the E value…

A

the more readily the reactions (as written) occurs

37
Q

The species that goes under oxidation, it is the stronger…

A

reducing agent

38
Q

The species that undergoes reduction is the stronger…

A

oxidizing agent

39
Q

How do you write a spontaneous reaction without a guide?

A
  1. reverse one of the HR into an oxidation step so the different of the electrode potentials gains a positive Ecell
  2. cathode minus anode = +Ecell
  3. reactants should be the stronger oxidizing/reducing agent
40
Q

How can metal displace other metals from solution? What is an example of this?

A

any metal that is lower in the list can reduce the ion of a metal that is higher up and thus displace that metal from solution; and E cell is overall positive

zinc can displace iron

41
Q

What metals can displacer H2 from water?

A

metals that are active enough to reduce H2O lie below that half-reaction

and if E cell is overall positive

42
Q

Faraday’s Constant:

A

9.65*10^4

43
Q

Equation of E cell given K

A

E cell = (0.0592/n) x logK

44
Q

Find K given the E cell:

A

log K = (n x Ecell) / 0.0592

45
Q

Describe the electron flow in a galvanic/voltaic cell:

A

the anode is negative because electrons are generated and the cathode is positive because electrons are removed

46
Q

Describe the electrons flow in the electrolytic cell:

A

external power source generates electrons for the cathode so it’s negative, and removes from the anode so it’s positive

47
Q

ELECTROLYSIS: Lysing of an aqueous solution means there’s a mixture of…

We compare the electrode potentials of […] to predict the electrode products.

A

ions and water; ions and water

48
Q

Overvoltage of water reduction and oxidtion:

A

0.4-0.6

Chemistry Lecture (7 decks)

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