Electrolytic cell
? >
Structure
what is
electrolysis
decomposition (-)
·
of a substance caused
by reductions occurs at cathode
the of electric oxidation anode (t)
passage
an current occurs at
·
Inert electrodes don't w/
·
react
>
what ?
is an
electrolyte electrolyte or reaction products
not spontaneous
· ·
a substance that can conduct
forming
free i o n s DC power source
electricity by
-
When molten or dissolved solution
[
Always anode to cathode electron
↓
flow
battery
2
I
!
Anode
& v cathode
2
2() (2 + 2e >
Natte Na
-
>
-
-
-
Nat Cl
NaCl
3
L
Positive electrode
Negative electrode
>
-
() lons more to (t) electrode >
-
>
-
lose electronsI are oxidised
>
they anions
-
are
-
D
e- Difference to Galvanic
⑭ ·
Needs
battery
endothermic
·
electrical to chemical
energy
-
Electrolysis of molten compound ·
Non-spontaneous
metal cathode Anode +
·
at ~
=
anode
·
·
non-metal at Cathode =
-
·
molten =
lons free to move * Galvanic is the opposite
electrolyte decomposes
·
electrical to chemical
energy Electrolysis of a salt solution
Contains 20 molecules & of salt
·
as well lons
Example
·
Hzolons compete with salt long
·
Alz03 water
E
1 will win when metals are weaker ox
Cathode & lose red
ag
ents when metals are
strong agents
2 H20tze >
-
He + 20t-
At
282-> 02 4 2 02
-
Al 3 + A
Halogen
+ > + 32 > 2 will
against
Cons win
-
S
.
02- A/3 +
water molecules
Anode >
they discharge readily
-
more
Alz 03 3 Water non-metal
will win
against lons
.
e Nos sol
g
.
? >
Structure
what is
electrolysis
decomposition (-)
·
of a substance caused
by reductions occurs at cathode
the of electric oxidation anode (t)
passage
an current occurs at
·
Inert electrodes don't w/
·
react
>
what ?
is an
electrolyte electrolyte or reaction products
not spontaneous
· ·
a substance that can conduct
forming
free i o n s DC power source
electricity by
-
When molten or dissolved solution
[
Always anode to cathode electron
↓
flow
battery
2
I
!
Anode
& v cathode
2
2() (2 + 2e >
Natte Na
-
>
-
-
-
Nat Cl
NaCl
3
L
Positive electrode
Negative electrode
>
-
() lons more to (t) electrode >
-
>
-
lose electronsI are oxidised
>
they anions
-
are
-
D
e- Difference to Galvanic
⑭ ·
Needs
battery
endothermic
·
electrical to chemical
energy
-
Electrolysis of molten compound ·
Non-spontaneous
metal cathode Anode +
·
at ~
=
anode
·
·
non-metal at Cathode =
-
·
molten =
lons free to move * Galvanic is the opposite
electrolyte decomposes
·
electrical to chemical
energy Electrolysis of a salt solution
Contains 20 molecules & of salt
·
as well lons
Example
·
Hzolons compete with salt long
·
Alz03 water
E
1 will win when metals are weaker ox
Cathode & lose red
ag
ents when metals are
strong agents
2 H20tze >
-
He + 20t-
At
282-> 02 4 2 02
-
Al 3 + A
Halogen
+ > + 32 > 2 will
against
Cons win
-
S
.
02- A/3 +
water molecules
Anode >
they discharge readily
-
more
Alz 03 3 Water non-metal
will win
against lons
.
e Nos sol
g
.
