Summary Chemistry Mind Map: Electrochemistry and Solutions

Electrochemical
ELECTROC
1 Cell 4 EMF of a cell 7 EMF; KC & ∆G
Left side Right side E0cell= E0Cathode-E0Anode 0 0
E cell= 0.0591 log KC, log KC=nE cell
Oxidation Reduction Ecell= RPCathode-RPAnode n
0.0591 Product formed
Anode Cathode Ecell= RPCathode+ OPAnode
∆G= -nFEcell m= EM
Negative Positive Ecell= OPAnode- OPCathode
x It
Spontaneous Non-spontaneous 96500
In cell, Cathode with high




PHYS
∆G<0 ∆G>0 EM= AM
Representation
2
RP ,Anode with low RP valency
makes spontaneous reactions 0 0
of cell E cell>0 E cell<0 1F=charge of 1 mole of
log KC>0 log KC<0 =96500 C

5
Zn| Zn2+|| Cu2+| Cu
Nernst equation
}
Ra| Pa|| Rc| Pc KC>1 KC<1 Na+ + e- → Na ⇒ 1F 1F
Mg2+ + 2e- → Mg ⇒ 2F 1
Galvanisation is applying pr
Product
at anode
Reactant
at cathode n [
Ecell= E0Cell- 0.0591 log Product
Reactant [ coating of Zn
Al3+ + 3e- → Al ⇒ 3F


Electrode potential (EMn+/M) For Zn| Zn2+|| Cu2+| Cu
E.P= Reduction Potential (R.P)
[
Ecell= E0Cell- 0.0591 log Zn2+ [
2+
= -Oxidation potential (O.P)




WALL
2 Cu
If R.P=x,then O.P=-x
For Ni| Ni || Ag | Ag
2+ +
Resistance(R)=
1 Electrolytic cell
Representation of Reduction half reaction:


[ [
M n+
+ ne -
M
Ecell= E0Cell- 0.0591 log Ni + 2
2+

2 (Ag ) Conductance(C)
Standard Reduction Potential(SRP)
(EOMn+/M) R1| P1|| R2| P2
R.P at 1M and 298K. ANODE CATHODE
If R2 then Ecell
Conductivity(K)
SRP is calculated by using SHE ,P1
•Anion goes to anode •Cation goes to cathode
Respresentation of SHE
•+ve electrode •-ve electrode Molar
H+(1M)| H2 | Pt(s) E0SHE=0
•Oxidation
,
(g,1 bar) •Reduction Conductivi
6 Application of
Nernst Equation
•A → A++e-
•A → An++ne-
•B+1e- → B-
•Bn+ne- → B- =1000 K

3 Electrochemical
series Electrode Potential
M
K→Scm-1
EMn+/M = E0Mn+/M- 0.0591 log 1
n [Mn+]
2 Product of electrolysis M→mol L-
→Scm2 m
Nernst equation in SHE Deposition order of cation: (order of R.P)
PH Li+ < K+ < Ca2+< Na+ < Mg2+ < Al3+ < Zn2+
1) EH+/H =-0.0591 log 2
< Fe2+ < Ni2+ < H+ < Cu2+ < Hg2+ < Ag+ < Au3+ 1Scm

2
2 [H+]2