Question

what is electrolycis​

Answer 1

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Electrolysis is the process of separating a compound into its constituent elements by passing electricity through it when in molten or aqueous state. The word electrolysis means splitting or breaking chemical substances with the help of electric current. For example, when electricity is passed through water containing a few drops of sulphuric acid, it breaks down to give its constituent elements as products i.e. hydrogen (H2) and oxygen (O2). Folllowing is the chemical equation for electrolysis of water :-

$\boxed{2H20=> 4H + O2}$

Answer 2

ELECTROLYSIS:-

Chemical decomposition produced by passing an electric current through a liquid or solution containing ions.

Various examples are there for this....

. Electrolysis of water

When electric current is put through water it splits the water molecules:

Cathode: 2H+(aq)+2e−→H2(g)Anode: 4OH−(aq)→O2(g)+2H2O+4e−Cathode: 2H+(aq)+2e−→H2(g)Anode: 4OH−(aq)→O2(g)+2H2O+4e−

2. Electrolysis of NaCl solution using Hg-electrode

NaCl solution is electrolyzed using Hg as cathode, and graphite as anode. Hg dissolves the formed Na and forms sodium amalgam, NaHg, which afterwards is reacted with water to get NaOH. On the anode chlorine gas is formed. This process is used to produce NaOH and chlorine gas on industrial scale.

Cathode: Na+(aq)+e−→Na(l)Anode: 2Cl−(aq)→Cl2(g)+2e−Cathode: Na+(aq)+e−→Na(l)Anode: 2Cl−(aq)→Cl2(g)+2e−

3. Electroplating

Electroplating is forming a thin, coherent metal layer on a metal object. For example using copper as anode, and a iron object as cathode in a CuSO4CuSO4 solution results in the oxidation of copper electrode and the deposition of copper on the iron object:

Cathode: Cu2+(aq)+2e−→Cu(s)Anode: Cu(s)→Cu2+(aq)+2e−Cathode: Cu2+(aq)+2e−→Cu(s)Anode: Cu(s)→Cu2+(aq)+2e−

4. Lead-acid battery

In a lead acid battery the redox reaction generates electricity, and the reverse charging process recharges the battery using external electrical power. Therefore the charging can be considered as 'electrolysis':

Cathode: PbSO4(s)+H+(aq)+2e−→Pb(s)+HSO−4Anode: PbSO4(s)+2H2O(l)→PbO2(s)+HSO−4(aq)+3H+(aq)+2e−Cathode: PbSO4(s)+H+(aq)+2e−→Pb(s)+HSO4−Anode: PbSO4(s)+2H2O(l)→PbO2(s)+HSO4−(aq)+3H+(aq)+2e−

Note, during charging the negative plate is the cathode and the positive plate is the anode, however during discharge the roles are reversed while the polarity of the plates remain. This is why the poles of the external power have to be connected to the same poles of the battery. Notice, that before charging both plates are in the PbSO4(s)PbSO4(s)form, and after charging the positive plate is in the PbO2(s)PbO2(s) and the negative plate is in the Pb(s)Pb(s) form.



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