For voltaic cells
3
* anode :
Oxidation/loses e 11-1 ,
OIL RIG in
electrolysis anodes (+ )
* cathode :
Oxidation Reduction reduction/gaise-/(t) +
cathodes (1)
is losing is gaining
CRA) 10A) ↑ For basic solutions , add OH-
0spon on soDon
to both sides to make #20
How to create half uxns that cancels
1) Dixide rxn Into 2 halves w/ Notation for VoltaicCell
Oxidized + reduced forms
2)
In/2n2
+
// (u21Cu A Whenever "NOS" of the
Balance atoms is a part equation
1) Balance Os by adding her
Her a YOU IGNORE becauseIt is part of salt bridge
4) Balance It's by adding H
+
writing a spontaneous ixn
1) Balance charge by adding e
-
#
a
X
Strength 1) whichever element is lower on potential list is
6) make sure
e-lost/gained your anode
are equal
OA
1) add rxns
Strength L
2) When you multiply rxns by a cresticient
Kathode) al
DON'T
estandard States
multiply Fall value
[ Ecell =
Ecathode -
Eanode
J A6
:
K Ecl RXn
*
207170 spontaneous Any element BELOW H2 , Hz0 ,
or
* F
in
O
Equilibrium
96485 J/mole-
g
=
so 20
Nonspontaneous anything above can DISPLACE It
Relationship between AG ; Ecll +
1
/JX
,
* AG is K
always in
16
:
M
↑
[16 nFEcl I
[AG -RTink
= -
=
Voltaic Cells vs Electrolytic Cells
-
>
spon (AG 0) nonspon (AG > O)
Early G
K canode (-1 >
- anode ( + /
cuthode( ) = cathode
[u = ink]
> +
-
(1)
~ Q =
(prob]
generate energy
creact]
: use
energy
Concentration +
cell Potential
3
> think
-
When Q ,
InQO ,
so Fall > Ecll
Of E cell
>
-
when Q =
1 ,
In Q =
0 , so Fall =
E all as Q
> when
- Q1 InQ70 , so Ecll (Fall
,
Stachiometry of Electrolysis
concentration Cells ·
[Eu 0592xxpH] =.
7
- anode has LOWER concentration
cathode has HIGHER concentration
[t miI =
*
standard-
nonstandard sprod A
E all [react] 3 "Q"
3
* anode :
Oxidation/loses e 11-1 ,
OIL RIG in
electrolysis anodes (+ )
* cathode :
Oxidation Reduction reduction/gaise-/(t) +
cathodes (1)
is losing is gaining
CRA) 10A) ↑ For basic solutions , add OH-
0spon on soDon
to both sides to make #20
How to create half uxns that cancels
1) Dixide rxn Into 2 halves w/ Notation for VoltaicCell
Oxidized + reduced forms
2)
In/2n2
+
// (u21Cu A Whenever "NOS" of the
Balance atoms is a part equation
1) Balance Os by adding her
Her a YOU IGNORE becauseIt is part of salt bridge
4) Balance It's by adding H
+
writing a spontaneous ixn
1) Balance charge by adding e
-
#
a
X
Strength 1) whichever element is lower on potential list is
6) make sure
e-lost/gained your anode
are equal
OA
1) add rxns
Strength L
2) When you multiply rxns by a cresticient
Kathode) al
DON'T
estandard States
multiply Fall value
[ Ecell =
Ecathode -
Eanode
J A6
:
K Ecl RXn
*
207170 spontaneous Any element BELOW H2 , Hz0 ,
or
* F
in
O
Equilibrium
96485 J/mole-
g
=
so 20
Nonspontaneous anything above can DISPLACE It
Relationship between AG ; Ecll +
1
/JX
,
* AG is K
always in
16
:
M
↑
[16 nFEcl I
[AG -RTink
= -
=
Voltaic Cells vs Electrolytic Cells
-
>
spon (AG 0) nonspon (AG > O)
Early G
K canode (-1 >
- anode ( + /
cuthode( ) = cathode
[u = ink]
> +
-
(1)
~ Q =
(prob]
generate energy
creact]
: use
energy
Concentration +
cell Potential
3
> think
-
When Q ,
InQO ,
so Fall > Ecll
Of E cell
>
-
when Q =
1 ,
In Q =
0 , so Fall =
E all as Q
> when
- Q1 InQ70 , so Ecll (Fall
,
Stachiometry of Electrolysis
concentration Cells ·
[Eu 0592xxpH] =.
7
- anode has LOWER concentration
cathode has HIGHER concentration
[t miI =
*
standard-
nonstandard sprod A
E all [react] 3 "Q"
