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Chem 30 > Chapter 13 > Flashcards

Chapter 13 Flashcards

(74 cards)

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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
stays colourless
not in the table of “common aqueous ions” in data booklet
26
anion movement
arrow pouting towards anode
27
action movement
arrow pointing towards cathode
28
electrons movement
arrow pointing to cathode (since electrons flow form anode to cathode)
29
inert electrodes definition and 2 examples
electrode that is made form a material not involved in the reaction Ex) Platinum (Pt) and graphite (C)
30
purpose of inert electrodes
are there to complete the circuit
31
cell notation: ll
salt bridge/ porous barrier
32
cell notation: l
phase boundary
33
in cell notation the ____ is always on the LEFT
anode
34
steps for cell notation
fill in
35
cell potential definition
electrical potential energy different between two charges
36
cell potential in voltaic cells definition
the electrical potential energy difference between two electrodes
37
factors affecting cell potential
- electrodes used - temp - concentration of electrolyte solutions - pressure (only if dealing with gases)
38
standard cell potential is measured using a ____
voltmeter
39
what is the reference electrode in the redox table
hydrogen
40
cell potential formula (and what is everything measured in)
Ecell= Ecathode - Eanode everything measured in volts
41
Ecell > O
reaction WILL proceed spontaneously (must be like this for voltaic)
42
Ecell< 0
reaction WON’T proceed spontaneously
43
steps for calculating standard cell potential
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
How to isolate for Er cathode
add Er anode to both sides
45
how to isolate for Er anode
fill in
46
when reference half cell is changed: reduction potentials ___ change
DO
47
when reference half cell is changed: cell potentials ___ change
DON’T
48
steps for determine potentials when reference cell is changed: CELL POTENTIAL
1) can still use hydrogen as régence electrode (so values in table DON’T change) 2) use standard cell formula to solve
49
steps for determine potentials when reference cell is changed: REDUCTION POTENTIAL
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
what is a battery
more than one cell connected together in a series
51
what is a primary battery
disposable battery
52
what is a secondary battery
rechargeable battery
53
what is a fuel cell
a type of cell that can be refuelled
54
what type of reactions are fuel cells
spontaneous
55
steps for determine half reactions in hydrogen fuel cells
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
two sources of hydrogen gas
- fossil fuels | - use of electricity to break apart compounds
57
what is corrosion
spontaneous reaction which occurs between compounds and their environment
58
example of good corrosion and why
oxidization of copper -copper oxide compound acts as a protective barrier for the copper beneath the surface
59
what is rust
the product of iron corrosion
60
what are the oxi and red half reactions of rust
oxi: Fe(s)—->Fe 2+ (aq) + 2e red: O2(g) + 2H20(l) + 4e ——> 4OH-(aq)
61
what is galvanizing
protective layer of zinc is placed over the iron
62
what is a sacrificial anode
material that is oxidized in order to prevent another material from being oxidized
63
what is allowed to be a sacrificial anode for something
can be any stronger reducing agent than the material it has to protect
64
cathodic protection
more reactive metal is placed over but doesn’t completely cover vulnerable metal replaced when oxidized
65
what is an electrolytic cell
a cell in which energy is used to power a NS reaction
66
electrolytic cells don’t have a _____
salt bridge
67
what is electrolysis
the NS splitting of a compound into its elements through the use of electric current
68
when does the chlorine anomaly occur
during the electrolysis of solutions containing chloride ions and water as the SOA’s
69
what happened during the chlorine anomaly
chlorine ions are oxidized (even though table shows water to be the SRA
70
secondary cells
rechargeable
71
example of a secondary cell
car battery
72
how do car batteries work
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
what is electroplating
process in which metal ions are reduced using an electric current to coat an electrode
74
what is Faraday’s law
the amount of substance produced or consumed in electrolysis is proportional to charge flowing through circuit

Chem 30 (6 decks)

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