Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII 1
Mass percentage (w/W)
,
Negative E° Stronger
2
A series of half–cells arranged in increasing Two copper strips dipped in an aqueous solution
standard oxidation potentials. reducing agent than Cu2+ + 2e–
of CuSO4 , then at Anode : Cu Painting, barrier protection, rust solutions
H+/H2 Cathode :Cu2+ + 2e– Cu
Rusting of iron, tarnishing of silver
Positive E° Weaker
U-shaped inverted reducing agent than H+/H2 Electrochemical phenomenon in
tube connecting Electronic conductance that:
two electrolytic which metal oxide of metal forms • Depends on Nature and structure of metal,
solution coating on metal surface. Number of valence electrons per atom,
• Temperature (Decreases
A chemical al s
Galvanic cell that converts h me t • with increase in temperature)
compound th ro u g
that dissociates energy of combustion of fuels ce
Cathode an
into ions and ct
u
like H 2, CH4 directly into Electrolytic (Ionic) Conductance:
conducts electric
nd
Reduction takes place electrical energy depends on:-
current ns
Co
Anode io Nature of electrolyte added,
ugh Size of ions solvation,
Oxidation takes place Electrode potential when c e thro
concentration of all species in r G° = –RT InK Conductan Nature of solvent and its viscosity,
half cell is unity. Concentration of electrolyte,
Temperature (increases with increase in
Co
Electrode : Pt coated with r G° = –n FE°cell nd Temperature)
e
u
Pt black, electrolyte : c ta
anc
nc
acidic solution pressure e
1 A A Unit : Siemens (S) or ohm–1 or mho
Half–cell 1 bar Pt(s) |H2(g)| H+(aq) Fuel cells C= = =
R l l
two portions of cell
Increases on dilution
Corrosion
2.303RT [M]
Inverse of Resist
Potential difference between Conductivity Ecell = E° cell – log n+
electrode and electrolyte. Cell nF [M ]
Relation 0.059 1
electrode
between Ecell = E°cell – log n+
l n [M ]
cell potential R=
Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII
A
and Gibbs = Resistivity
energy Unit : Ohm – Meter
Daniell Cell :Cathode: Copper, Anode : Z inc; Salt nE° cell
Electroch KC = Antilog
bridge : Agar agar; electrolyte : KCN/KNO3 emic 0.0591
al : Mn+(aq) + ne– M(s)
Reduction : Cu2+(aq) + 2e Cu (s) chemical De 2.303 RT
ener vic E°cell = log K C
Oxidation : Zn(S) Zn2+(aq) + 2e gy
to ec nF
2+ ele o
Zn|Zn (C1) || Cu 2+(C2)|Cu
nv
c tr
i Electrical
er
V
ca
1. Calculate °m for any electrolyte from ° of individual ions
l
resistance R= Unit : Ohm ( )
tin
g
en
rG° = –RT lnK I 2. Determine value of dissociation constant for weak electrolytes
e rg
Nernst
y
equation
° Limiting molar conductivity of an electrolyte can be represented as
rG° = –n FE cell Nature of material sum of individual contribution of anions and cations of the electrolyte
Types of being electrolysed °m = v+ °++v– °–
Cells Resistance
Types of electrodes Kohlrausch's law of independent migration of ions
Relation between cell
potential and Gibbs
energy Products of Weak electrolyte
Strong electrolyte Ù
electrolysis ½ = m (acetic acid)
depends upon m= m – AC (KCl) Ù°m
1st Law Amount of substance in a chemical reaction which occurs at any
electrode during electrolysis by a current is proportional to the o ch e m i s A
quantity of electricity passed through electrolyte W = ZIt ctr t m= m; = V
l
ry
nd Limiting molar conductivity :If molar conductivity
Ele
2 Law Amount of different & s ubstances liberated by same quantity of
reaches a limiting value when concentration
electricity passing through electrolytic solution are proportional
Molar conductivity: Conductance of approaches zero. C 0, m = m
to their chemical equivalent weights …… W1 W2 W3
volume V of solution containing 1 mole of
E1 E2 E3
Faraday’s laws electrolyte kept between two electrodes with Trace the Mind Map
of electrolysis area of cross section A and distance of unit length
First Level Second Level Third Level
Mass percentage (w/W)
,
Negative E° Stronger
2
A series of half–cells arranged in increasing Two copper strips dipped in an aqueous solution
standard oxidation potentials. reducing agent than Cu2+ + 2e–
of CuSO4 , then at Anode : Cu Painting, barrier protection, rust solutions
H+/H2 Cathode :Cu2+ + 2e– Cu
Rusting of iron, tarnishing of silver
Positive E° Weaker
U-shaped inverted reducing agent than H+/H2 Electrochemical phenomenon in
tube connecting Electronic conductance that:
two electrolytic which metal oxide of metal forms • Depends on Nature and structure of metal,
solution coating on metal surface. Number of valence electrons per atom,
• Temperature (Decreases
A chemical al s
Galvanic cell that converts h me t • with increase in temperature)
compound th ro u g
that dissociates energy of combustion of fuels ce
Cathode an
into ions and ct
u
like H 2, CH4 directly into Electrolytic (Ionic) Conductance:
conducts electric
nd
Reduction takes place electrical energy depends on:-
current ns
Co
Anode io Nature of electrolyte added,
ugh Size of ions solvation,
Oxidation takes place Electrode potential when c e thro
concentration of all species in r G° = –RT InK Conductan Nature of solvent and its viscosity,
half cell is unity. Concentration of electrolyte,
Temperature (increases with increase in
Co
Electrode : Pt coated with r G° = –n FE°cell nd Temperature)
e
u
Pt black, electrolyte : c ta
anc
nc
acidic solution pressure e
1 A A Unit : Siemens (S) or ohm–1 or mho
Half–cell 1 bar Pt(s) |H2(g)| H+(aq) Fuel cells C= = =
R l l
two portions of cell
Increases on dilution
Corrosion
2.303RT [M]
Inverse of Resist
Potential difference between Conductivity Ecell = E° cell – log n+
electrode and electrolyte. Cell nF [M ]
Relation 0.059 1
electrode
between Ecell = E°cell – log n+
l n [M ]
cell potential R=
Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII
A
and Gibbs = Resistivity
energy Unit : Ohm – Meter
Daniell Cell :Cathode: Copper, Anode : Z inc; Salt nE° cell
Electroch KC = Antilog
bridge : Agar agar; electrolyte : KCN/KNO3 emic 0.0591
al : Mn+(aq) + ne– M(s)
Reduction : Cu2+(aq) + 2e Cu (s) chemical De 2.303 RT
ener vic E°cell = log K C
Oxidation : Zn(S) Zn2+(aq) + 2e gy
to ec nF
2+ ele o
Zn|Zn (C1) || Cu 2+(C2)|Cu
nv
c tr
i Electrical
er
V
ca
1. Calculate °m for any electrolyte from ° of individual ions
l
resistance R= Unit : Ohm ( )
tin
g
en
rG° = –RT lnK I 2. Determine value of dissociation constant for weak electrolytes
e rg
Nernst
y
equation
° Limiting molar conductivity of an electrolyte can be represented as
rG° = –n FE cell Nature of material sum of individual contribution of anions and cations of the electrolyte
Types of being electrolysed °m = v+ °++v– °–
Cells Resistance
Types of electrodes Kohlrausch's law of independent migration of ions
Relation between cell
potential and Gibbs
energy Products of Weak electrolyte
Strong electrolyte Ù
electrolysis ½ = m (acetic acid)
depends upon m= m – AC (KCl) Ù°m
1st Law Amount of substance in a chemical reaction which occurs at any
electrode during electrolysis by a current is proportional to the o ch e m i s A
quantity of electricity passed through electrolyte W = ZIt ctr t m= m; = V
l
ry
nd Limiting molar conductivity :If molar conductivity
Ele
2 Law Amount of different & s ubstances liberated by same quantity of
reaches a limiting value when concentration
electricity passing through electrolytic solution are proportional
Molar conductivity: Conductance of approaches zero. C 0, m = m
to their chemical equivalent weights …… W1 W2 W3
volume V of solution containing 1 mole of
E1 E2 E3
Faraday’s laws electrolyte kept between two electrodes with Trace the Mind Map
of electrolysis area of cross section A and distance of unit length
First Level Second Level Third Level
