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Chem 30 > Chapter 13 > Flashcards

Chapter 13 Flashcards

1
Q

electrochemical cells include ____ and ___ cells

A

voltaic and electrolytic cells

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2
Q

voltaic cells are always ______

A

spontaneous

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3
Q

voltaic cells use _____ to transform ____ into _____

A

redox reactions

chemical potential energy

electrical energy

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4
Q

voltaic cell process

A

electrodes are spectated and the electrons lost by the one electrode flow in one direction (producing electrical current) towards the other electrode

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5
Q

what are the anode and cathode in the voltaic cell diagram

A

the solid sticks

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6
Q

cathode definition

A

electrode where reduction occurs

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7
Q

cathode charge

A

positive

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8
Q

anode definition

A

electrode where oxidization occurs

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9
Q

anode charge

A

negative

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10
Q

external circuit definition

A

wire connecting anode to cathode

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11
Q

electrons travel from ___ to ____

A

anode to cathode

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12
Q

salt bridge/ porous cup definition

A

maintains the electro neutrality of solutions

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13
Q

salt bridge/ porous cup doesn’t allow _____

A

the ions of the two cell solutions from coming into contact with the opposite electrode

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14
Q

why must the salt bridge be carefully selected

A

so it doesn’t precipitate out any of the ions of the cell solution

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15
Q

the salt bridge is composed of ____ and ___

A

anions and cations

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16
Q

anions definition

A

negative ions, travel towards the anode

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17
Q

cations definition

A

positive ions, travel towards the cathode

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18
Q

electrolyte definition

A

something in solution

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19
Q

steps for determining anode and cathode in voltaic cell

A

1) determine SOA and SRA
- list everything you have and consult redox table

2) assign anode and cathode
- anode=where oxidization occurs
- cathode=where réductions occurs

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20
Q

steps for determining half reactions in voltaic cell (and note for steps 1 and 2)

A

1) write out half reaction of anode
- from redox table

2) write out half reaction of cathode
- from redox table

3) determine SOA and SRA based on ON’s of half reactions
4) write out oxi half reaction
5) write out red half reaction
* for steps 1 and 2: write reactions in regular way

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21
Q

decrease in mass

A

the one being oxidized (since it’s losing electrons)

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22
Q

increase in mass

A

the one being reduced (since it’s gaining electrons)

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23
Q

brighter colour

A

the one being oxidized

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24
Q

paler colour

A

the one being reduced

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25
Q

stays colourless

A

not in the table of “common aqueous ions” in data booklet

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26
Q

anion movement

A

arrow pouting towards anode

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27
Q

action movement

A

arrow pointing towards cathode

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28
Q

electrons movement

A

arrow pointing to cathode (since electrons flow form anode to cathode)

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29
Q

inert electrodes definition and 2 examples

A

electrode that is made form a material not involved in the reaction

Ex) Platinum (Pt) and graphite (C)

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30
Q

purpose of inert electrodes

A

are there to complete the circuit

31
Q

cell notation: ll

A

salt bridge/ porous barrier

32
Q

cell notation: l

A

phase boundary

33
Q

in cell notation the ____ is always on the LEFT

A

anode

34
Q

steps for cell notation

A

fill in

35
Q

cell potential definition

A

electrical potential energy different between two charges

36
Q

cell potential in voltaic cells definition

A

the electrical potential energy difference between two electrodes

37
Q

factors affecting cell potential

A
  • electrodes used
  • temp
  • concentration of electrolyte solutions
  • pressure (only if dealing with gases)
38
Q

standard cell potential is measured using a ____

A

voltmeter

39
Q

what is the reference electrode in the redox table

A

hydrogen

40
Q

cell potential formula (and what is everything measured in)

A

Ecell= Ecathode - Eanode

everything measured in volts

41
Q

Ecell > O

A

reaction WILL proceed spontaneously (must be like this for voltaic)

42
Q

Ecell< 0

A

reaction WON’T proceed spontaneously

43
Q

steps for calculating standard cell potential

A

1) write red and oxi half reactions
- determine OA and RA using redox table

2) determine anode and cathode
3) write down reduction potentials from data booklet
4) use standard cell formula to solve for unknown

44
Q

How to isolate for Er cathode

A

add Er anode to both sides

45
Q

how to isolate for Er anode

A

fill in

46
Q

when reference half cell is changed: reduction potentials ___ change

A

DO

47
Q

when reference half cell is changed: cell potentials ___ change

A

DON’T

48
Q

steps for determine potentials when reference cell is changed: CELL POTENTIAL

A

1) can still use hydrogen as régence electrode (so values in table DON’T change)
2) use standard cell formula to solve

49
Q

steps for determine potentials when reference cell is changed: REDUCTION POTENTIAL

A

1) identify new reference half cell and write out half reaction
2) subtract/ add appropriate # to make sure E of reference cell is 0
3) write out half reactions of other
4) do the same thing you did to the E of the reference cell to the E of the other

50
Q

what is a battery

A

more than one cell connected together in a series

51
Q

what is a primary battery

A

disposable battery

52
Q

what is a secondary battery

A

rechargeable battery

53
Q

what is a fuel cell

A

a type of cell that can be refuelled

54
Q

what type of reactions are fuel cells

A

spontaneous

55
Q

steps for determine half reactions in hydrogen fuel cells

A

1) determine anode and cathode (if not given)
- can figure out through electron flow (anode to cathode)

2) write out oxi half reaction
- oxi occurs at anode

3) write out red half reaction
- red occurs at cathode

56
Q

two sources of hydrogen gas

A
  • fossil fuels

- use of electricity to break apart compounds

57
Q

what is corrosion

A

spontaneous reaction which occurs between compounds and their environment

58
Q

example of good corrosion and why

A

oxidization of copper

-copper oxide compound acts as a protective barrier for the copper beneath the surface

59
Q

what is rust

A

the product of iron corrosion

60
Q

what are the oxi and red half reactions of rust

A

oxi: Fe(s)—->Fe 2+ (aq) + 2e
red: O2(g) + 2H20(l) + 4e ——> 4OH-(aq)

61
Q

what is galvanizing

A

protective layer of zinc is placed over the iron

62
Q

what is a sacrificial anode

A

material that is oxidized in order to prevent another material from being oxidized

63
Q

what is allowed to be a sacrificial anode for something

A

can be any stronger reducing agent than the material it has to protect

64
Q

cathodic protection

A

more reactive metal is placed over but doesn’t completely cover vulnerable metal

replaced when oxidized

65
Q

what is an electrolytic cell

A

a cell in which energy is used to power a NS reaction

66
Q

electrolytic cells don’t have a _____

A

salt bridge

67
Q

what is electrolysis

A

the NS splitting of a compound into its elements through the use of electric current

68
Q

when does the chlorine anomaly occur

A

during the electrolysis of solutions containing chloride ions and water as the SOA’s

69
Q

what happened during the chlorine anomaly

A

chlorine ions are oxidized (even though table shows water to be the SRA

70
Q

secondary cells

A

rechargeable

71
Q

example of a secondary cell

A

car battery

72
Q

how do car batteries work

A

battery is acting as a voltaic cell when you start it (producing electricity from chemical POTENTIAL energy)

battery is acting as an electrolytic cell when you run in (electricity is being converted into chemical POTENTIAL energy)

73
Q

what is electroplating

A

process in which metal ions are reduced using an electric current to coat an electrode

74
Q

what is Faraday’s law

A

the amount of substance produced or consumed in electrolysis is proportional to charge flowing through circuit

Chem 30 (6 decks)

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