electrochemical cells
DESCRIPTION
A set of slides created to teach Electrochemical Cells to learners at Bishops Diocesan College in Cape Town.TRANSCRIPT
ELECTROCHEMICAL CELLS
K Warne
Electrochemical Cell.
Two metals can react indirectly.
Cu2+ + 2e- Cu
Zn2++ 2e- --> Zn
Cu2+ + 2e-
--> CuAttract elelctons strongly
Attract elelctons weakly
OXIDISING AGENT
REDUCING AGENT
Top right reacts
with bottom left.
_
_
_
_
_
Zn
_
_
Cu
V
_
KNO3(aq)
+
>
Zn Zn2+ + 2e-
CuSO4ZnSO4
Salt bridge
anodecathode
Zn + Cu2+ Zn2+ + Cu
oxidation reduction
REDUCING AGENT OXIDISING AGENT
e-
WORKED EXAMPLES
1. The redox couples Mn2+(aq) Mn(s) and U3+(aq) U(s) have
Eθ values of –1.18 and –1.79 respectively. Determine Eθcell
when they are combined and write an equation for the
reaction that takes place.
Eθcell = Eθ
O.A. - EθR.A. = -1.18 – (-1.79) = +0.61v
3Mn2+(aq) + 2U(s) 3Mn(s) + 2U3+(aq)
2. The redox couples Co2+(aq) Co(s) and Ni2+(aq) Ni(s)
have Eθ values of –0.28v and –0.23v respectively. Write
an equation for the spontaneous reaction and use the Eθ
values to justify your answer.
Co(s) + Ni2+(aq) Co2+(aq) + Ni(s)
Eθ = EθO.A - Eθ
R.A = -0.23 – (-0.28) = +0.05v
Ni2+(aq) + Co(s) Co2+(aq) + Ni(s)
Electrolytic cell: Converts electrical energy to chemical energy.
Copper chloride
CuCl2
+-
Cu2+
Cl-
Cu2+(aq)+ 2e-
Cu(s)
REDUCTION
CATHODE
2Cl-(aq) Cl2(g) + 2e-
OXIDATION
Anode
Electrolysis – Electrolytic Cell
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> ScienceCafe
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
STANDARD HYDROGEN ELECTRODE
……….. electrode
H2 gas pressure of ……….
(………. kPa)
Solution of …..M H+ ions
(HCl)
…………K
Eθ = ……………v
S.H.E. is ………. to set up.
……………….. standard
electrodes used.
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
DETERMINATION OF CELL POTENTIALS
Eθ values are determined using a ……………………………… electrode.
The S.H.E is always the …………………. electrode.
Standard Conditions : ………………………………………………….
A secondary standard electrode the ………………. electrode can be used.
Eθcell= …………………………………………
Eθcell= ………………. – ……….
N+(aq)
N+(s)
Unknown electrodeStandard electrode
High resistance voltmeter
Salt bridge
If a cell potential of
1.45v is obtained
with metal N. Then
the electrode
potential of N+ /N is
..................................
..................................
..................................
..................................
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Electrolysis in aqueous solutions
Na+ + e- Na -2.71
Mg2+ + 2e- Mg -2.37
2H2O + 2e- H2 + 2OH - -0.83
Cu2+ + 2e- Cu +0.34
H2 + 2e- 2H+
SO42- + 4H+ + 2e- SO2 +0.17
H2O + O2 + 2e- 4OH- +0.40
Cl2 + 2e- 2Cl- +1.36
+
-Cathode: Reduction
Cu2+ + 2e- Cu
Anode: Oxidation
Cl2 + 2e- 2Cl-
The most
positive system
present will
react at the
cathode
?Which ions will
react at which
electrodes?
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Cathode
( )
Copper
chloride
CuCl2
+-
Cu2+
Cl-
Cu2+(aq)+ 2e-
Cu(s)
REDUCTION
CATHODE
(-)
2Cl-(aq) Cl2(g) + 2e-
OXIDATION
Anode
(+)
_
_
_
_
_
Zn
_
_
Cu
V
KNO3(aq)
+
>
Zn Zn2+ + 2e-
CuSO4
ZnSO4
Salt
bridge
Anode
(-)
Zn + Cu2+ Zn2+ + Cu
oxidation reduction
REDUCING
AGENTOXIDISING
AGENT
e-
_
Cu2+ + 2e- Cu
Chemical Energy Electrical Energy
+e-
Electrochemical Cells
Voltaic (Galvanic) vs Electrolytic
Electrical
Energy
Chemical
Energy
Electrical Energy Chemical Energy
Electrical
Energy
Chemical
Energy
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Electrolysis of aqueous solutions (MX)
(H2O)
M+
(Metal ion)
X-
(Non-Metal
ion)
- +
If the metal is more positive than
hydrogen, its ions will be reduced.
M+ + e M
If halide ions (X-) are present (more
positive than OH- ) ions then the
halide ions (X-) are oxidised.
X- X2 + 2e-
SAMPLE ONLY SAMPLE ONLY
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Electrolysis - Lead Bromide
PbBr2
PbBr2 (Heat) Pb2+ + Br-
Pb2+(l) + 2e-
Pb(l) 2Br - (l) Br2(g) + 2e-
Pb2+(l) + 2Br -(l) Pb(l) + Br2(g)
+-
electrons
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Electrolysis – Sodium chloride
2H2O + 2e- H2 + 2OH- 2Cl- Cl2 + 2e-
2H2O + 2Cl- + (2Na+) Cl2 + H2 + 2OH- + (2Na+)
SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY
For FULL presentation click HERE >> www.warnescience.net
Hi…
This is a SAMPLE presentation only.
My FULL presentations, which contain a lot more slides and other resources, are freely available
on my resource sharing website:
www.warnescience.net(paste into your browser if link above does not work)
Have a look and enjoy!
Keith Warne
WarneScience