Summary
Summary Electrochemistry study notes
- Course
- Physical Sciences
- Institution
- 12th Grade
An in-depth document filled with explanations, practice questions, examples and more. all grade 12 learners must have.
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ELECTROCHEMISTRY :Galvanic Cell : * oxidation =
top right
↳ torch cells car batteries * reduction = bottom left
↳
,
conversion of chemical potential electrical
energy to
energy
↳ self-sustaining electrode reactions
↳ produce elec tric cur rent
Anode : the electrode where oxidation takes place (an ox)
Cathode : the electrode where reduction takes place (red cat)
Electrolyte :
a substance that can conduct electricity by forming free ions When Motten or dissolved in solution
external Ce- moves from -
to +
circuit
-
J
e
e-
-
always on left
-
anode (oxidation) ·
Cathode (reduction)
C -
) Salt bridge
Ch
-
KNOz/k(I ↳
? & 2n
Cul +
Cu
S 2e-
7
In 22- +
In . +
ions-
M internal
, loses mass circuit
is gains
Y mass
build
> e-won't flow
no
pote,
current
inzt
Soy
2+
build up
>
no
of 11
e-won't flow
current
21 S 04
5042- CU
cusne
&
·
electrolyte
·
more reactive kichs less reactive out of solution
·
no conventional current
cgrp1 metals +
·
Salt bride made up of any soluble ionically bonded Salt (conduct electricity in solution
= can't have In /Cu/S042-
i
I can't be halogen forms precipitate (stops reaction)
·
cell notation :
Ote :
25 C
%
nus) In caq) Cimo .
am-3) /l Cusai Limo am .
*
). Cu is)
·
Electrons flow in External circuit
T
phase
boundary reducing agent/ oxidised species // oxidising agent/reduced species "Tony flow in Internal circuit
*
· -
cell
=
E Cathode -
Eanode
=
(+ 0, 34) -
1 -
0, 76)
= I
,
IV
7
1
(H) =
Spontaneous
: if ( ) -
Set up wrong , switched
,-salt
bridge :
maintains electrical neutrality in the half-cells
completes the circuit * anious from cathode electrode more into allock electrode
Standard conditions :
Aqueous solution =
Imol .
am s
temperature =
25 %
(1 x105kPa)
·
01
gases 1atm
=
,
Standard electrode potentials :
= cell
=
E cathode -
EGanode
energy conversion :
chemical potential >
--
electrical
takes place
>
-
added energy
Ecell) o =
Spontaneous
wo
↳ exothermic
E cell <a =
non-spontaneous
celi notation :
>
electrodes on outside
-
~ =
phase boundary ,
btwn 2 chemical species -
diff phases but in contact
C =
salt bridge
·
Oxidised
reducing agent. species oxidising agent reduced species
+
11 Cu2 /Cu
+
e .
g. In/In"
↳When both chemical
species in same phase
↳ separate by comma
Ptiss Sn
"Yeg) sn't Il
fest fet P
a
*
,
,, ,
,
, Galvanic cell
num
↳
spontaneous
↳ exothermic
Imature
·
2 half-cells
an anode Solid/liquid/gas)
·
(neg. cell-oxidation -
·
a lathode /pos cell-reduction
·
-
Solid/liquid/gas)
an electrolyte in each half cell (containsions of
oxidisinga reducing agents respective half-cells
·
in
·
an electrode in each half cell
a salt bridge connecting the half cells
·
2
the salt bridge :
↳ filled salt solution
with a saturated
↳ common : KC1 , NaCl , KNOs ,
NacSO4
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