Tab 1
, Electrochemistry
● Process in which a non-spontaneous reaction happens when DC current is
passed through an electrolyte(molten/aqueous).
● Products of electrolysis:-
1. Type of Electrodes:-
a) Active Electrodes: At cathode, metal ions from electrolyte
are reduced and at anode, metal ions from the anode are
oxidised,i.e, at cathode ions convert to solid state and at
anode solid converts to ions.
b) Inert Electrodes: At cathode and anode, metal ions from the
electrolyte get reduced and oxidised respectively.
2. Over-potential: Sometimes, thermodynamically feasible reactions
might not take place due to over-potential. So, in such cases, the
kinetically faster reaction takes place.
3. Reduction Potentials:
a) At cathode, the ion/molecule with highest E0reduction is reduced.
b) At anode, the ion/molecule with lowest E0reduction is oxidised.
● Faraday’s Laws:-
1. First Law: The amount of substance formed at a respective
electrode is directly proportional to the amount of charge passed
through the electrolyte.
2. Second Law: When the same quantity of charge is passed through
different electrolytes connected in series, the amount of substance
obtained at the respective electrodes is directly proportional to the
eq. Mass of the respective substances.
● Electrical Resistance, Conductance, Resistivity, Conductivity:-
1. Conductance: Reciprocal of resistance.
2. Conductivity: Conductance offered by a conductor of 1m length
and 1m2 cross sectional area.
OR
Conductance of all ions produced by a given weight of electrolyte
when dissolved in a unit volume of solution.
● Molar Conductivity:- The conductance of all ions produced in 1 mole of
electrolyte in a given volume of solution.
● Limiting Molar Conductivity:- The molar conductivity at infinite dilution or
c→0.
, Electrochemistry
● Process in which a non-spontaneous reaction happens when DC current is
passed through an electrolyte(molten/aqueous).
● Products of electrolysis:-
1. Type of Electrodes:-
a) Active Electrodes: At cathode, metal ions from electrolyte
are reduced and at anode, metal ions from the anode are
oxidised,i.e, at cathode ions convert to solid state and at
anode solid converts to ions.
b) Inert Electrodes: At cathode and anode, metal ions from the
electrolyte get reduced and oxidised respectively.
2. Over-potential: Sometimes, thermodynamically feasible reactions
might not take place due to over-potential. So, in such cases, the
kinetically faster reaction takes place.
3. Reduction Potentials:
a) At cathode, the ion/molecule with highest E0reduction is reduced.
b) At anode, the ion/molecule with lowest E0reduction is oxidised.
● Faraday’s Laws:-
1. First Law: The amount of substance formed at a respective
electrode is directly proportional to the amount of charge passed
through the electrolyte.
2. Second Law: When the same quantity of charge is passed through
different electrolytes connected in series, the amount of substance
obtained at the respective electrodes is directly proportional to the
eq. Mass of the respective substances.
● Electrical Resistance, Conductance, Resistivity, Conductivity:-
1. Conductance: Reciprocal of resistance.
2. Conductivity: Conductance offered by a conductor of 1m length
and 1m2 cross sectional area.
OR
Conductance of all ions produced by a given weight of electrolyte
when dissolved in a unit volume of solution.
● Molar Conductivity:- The conductance of all ions produced in 1 mole of
electrolyte in a given volume of solution.
● Limiting Molar Conductivity:- The molar conductivity at infinite dilution or
c→0.
