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
The benefits of buying summaries with Stuvia:
Guaranteed quality through customer reviews
Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.
Quick and easy check-out
You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.
Focus on what matters
Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!
Frequently asked questions
What do I get when I buy this document?
You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.
Satisfaction guarantee: how does it work?
Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.
Who am I buying these notes from?
Stuvia is a marketplace, so you are not buying this document from us, but from seller sydneyystuartt. Stuvia facilitates payment to the seller.
Will I be stuck with a subscription?
No, you only buy these notes for $3.94. You're not tied to anything after your purchase.