Application of Electrochemical

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Application of Electrochemical

Published by: Nuru

Published date: 26 Jun 2021

Application of Electrochemical in Grade 12

Application of Electrochemical or Emf or Activity Series

Application of Electrochemical are as follows:

  1. To compare the relative oxidizing and reducing powers- The magnitude of the standard reduction potential of metal or nonmetal gives a measure of its tendency to lose the electrons to get oxidized and hence to act as a reducing agent. Greater the value of standard reduction potential of a given species greater its tendency to gain the electron to undergo reduction and hence act as the oxidizing agent. F2 has the highest standard reduction potential and Li+ ion has the lowest standard reduction potential it means F2 is reduced most easily but Li+ ion is reduced with the greatest difficulty. Therefore F2 is the strongest oxidizing agent and Li+ ion is the weakest oxidizing agent. Greater the value of standard reduction potential of a given species, smaller its tendency to lose the electron to undergo oxidation and leave the electron to undergo oxidation and hence act as reducing agent. Li will be oxidized most easily and hence it is the best reducing agent but F– is oxidized with the greatest difficulty and hence it is the weakest reducing agent.

2. To compare the relative activity of metals- Smaller the standard reduction potential of metal, the more easily it can lose the electron, and hence, the greater is its reactivity thus a metal with lower reduction potential can displace metal with higher reduction potential from the salt solution.

3. To calculate EMF of given galvanic cell- Galvanic cell is based on a reaction which can be observed into two half-reaction

  • Oxidation half-reaction
  • Reduction half-reaction

The emf of the galvanic cell can be given as:-

EMF of cell= standard electrode potential of cathode- standard electrode potential of the anode

i.e. E degree of cell= Eocathode – Eoanode

4. To predict whether a metal will produce Hydrogen gas from dilute acid or not- A metal that has a strong tendency to lose an electron to form metal ions will displace H+ ions from the acid solution and thus will produce hydrogen gas.

M(s) + 2H+(from dil.acid)→H++(aq) + H2↑

Greater the value of standard reduction potential of metal smaller its tendency to lose the electrons to form metal ions and hence smaller its tendency to displace H+ ions or form water to produce hydrogen gas.

5. To see whether a given redox reaction is feasible or not EMF of the cell based on the given redox reaction is calculated. If EMF is found to be positive then the Galvanic cell does work and if EMF is found to be negative then given Galvanic does not work.

Therefore the Application of Electrochemical or Emf or Activity Series has explained above.