1. CLASS 12
KV Pitampura

2. ELECTRODE POTENTIAL
 It is the difference between the electrodes (
reeduction potentials) of the cathode and anode.
 It is also called the EMF.
ACTIVITY SERIES
 it is list of elements like metals or non-metals in
which elements are arranged in order of their
relative reactivity

4. CELLREACTION
 The cell reaction is the overall reaction which takes
place in the cell, written on the assumption that the
right hand electrode is the cathode,
 i.e. assuming that the spontaneous reaction is the one
in which reduction is occurring in the right-hand
compartment.
overall reaction
Zn(S) + Cu2+ → Zn2+
(aq) + Cu(s)
Cell Representation →Zn/Zn2+//Cu2+/Cu
Oxidation: Zn(S) →Zn2+
(aq) + 2e- (Anode)
Reduction: 2e- + Cu2+
(aq) → Cu(s) (Cathode)

5. E°cell: Standard Cell Potential
 E°cell is the electromotive force (also called
cell voltage or cell potential) between two
half-cells.
 E°cell is measured in volts (V).
Eo cell=Eo cathode−Eo anode

6. Ecell OR EMF
 The cell potential is the difference between the
electrode potentials (reduction potentials) of the
cathode and anode. I
 t is called the cell electromotive force (emf) of the cell
when no current is drawn through the cell.
Ecell=Ecathode−Eanode

7.  The Nernst equationwas named after the German
chemist Walther Nernstwho establishedvery
useful relations between the energy or potential
of a cell to the concentrations of participating
Ions.
⇒
][
][
ln
Fn
R T
-EoE
cathode
anode

][
][
log
Fn
2.303RT
-EoE
cathode
anode


8. NUMERICAL
][
]Mg2+[
log
F2
R T
-cellEoE


Ag
][(0.0001)2
]0.130[
log
F2
0.059
-3.17E
Ecell=3.17V−0.21V
Ecell=+2.96V.
Represent the cell in which the following reaction
takes place Mg(s) + 2Ag+ (0.0001M) → Mg2+ (0.130
M) + 2Ag(s) Calculate its Ecell if Eo cell = 3.17 V.
Q
Ans

9. NCERT
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