CHE 101 Chapter Notes - Chapter 12: Redox, Electrochemistry, Electric Current
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Revision Notes on Redox Reactions and Electrochemistry:
Electrochemistry is the branch of chemistry which deals with the chemical changes caused in the
matter by passage of electric current and conversion of chemical energy into electrical energy and
Conductors and Non Conductors
Substances around us can be divided into two classes based on their ability of conduct electricity:
●Non-Conductors: Those substances which do not allow electric current to pass through
them are called non-conductors or insulators. Example: - wood, plastic glass, rubber etc.
●Conductors: Those substances which allow electric current to flow through tem are
called conductors. Examples: Copper, Iron, Gold, Silver, Graphite, salt solution etc.
Conductors can further be divided into two groups
●Metallic Conductors: These conductors conduct electricity or electric current by
movement of electrons without undergoing any chemical change during the process.
These conduct electricity in both solid as well as molten state. Example: All the metals
●Electrolytes: Those substances which conduct electricity only when they are present in
aqueous solution and not in solid form are called electrolytes. These conduct electricity by
movement of ions in solutions.
Comparison of Electrolytic and Metallic Conduction
Specific Resistance or resistivity (ρ):
R = ρ× l /A
R = Resistance
A=Area of cross sections of electrodes
l = Distance between the electrodes.
Specific Conductance or Conductivity (κ):
κ = 1/ ρ
Units: W–1 cm–1 or Sm–1
Electric current flows by movement of
Electric current flows by movement of ions.
No chemical change occurs.
Ions are oxidized or reduced at the electrodes.
It does not involve the transfer of any
It involves transfer of matter in the form of ions.
Ohm's law is followed.
Ohm's low is followed.
Resistance increases with increase of
Resistance decreases with increase of
Faraday law is not followed.
6Faraday law is followed.
Equivalent Conductance (Λ):
Conducting power of all the ions produced by one g-equivalent i.e. one equivalent of an electrolyte in a
Λ = 1000 κ /C
Where, C be the normality of solution i.e. concentration of electrolytic solution in equivalent/L.
Molar Conductance (Λm):
Conductance of solution due to all the ions produced by one mole of the dissolved electrolyte in a given
Λm = κ/c
Where, c = concentration of solution in mol m-3.
Λm = κ×1000/M
Where, M is molarity of solution.
Units: S cm2 mol-1
Relation between Λ and Λm
Λm = n Λ
Where n = n-factor of the electrolyte = total charge carried by either ion = M/E
Variation of Conductance with Dilution:
Specific conductance: Decrease with dilution due to decrease in number of ions per c.c. of the solution.
Molar and Equivalent Conductance: Increases with increase in dilution.
● Weak electrolyte: Increase is due to increase in extent of ionization.
●Strong electrolyte: Increase is due to increase in mobility of ions because of decreased
Λm = Λ0m – (A+B Λ0m) √C