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What is electr­olysis?

Electr­olysis can be defined as the decomp­osition of compounds which happens when direct current passes through a solution or molten compound.

Terms used in electr­olysis

Electr­olyte
This can be defined as a liquid which conduct elections.
Types of electr­olyte
Strong Electr­olyte: These are strong acids and strong bases/­alk­ali's.
Weak Electr­olyte: These are weak acids and weak bases/­alk­ali's.
Electrode
This is a metal rod, plate or wire, which conducts electr­icity in an electr­olytic cell.
Anode: This is the positive electrode through which conven­tional current enters and electrons leave.
Cathode: This is the negative electrode through wich conven­tional current leaves and electrons enter.
Electr­olytic Cell
This is the setup of two electr­odes, placed in an electr­olyte, used in the electr­olysis of substa­nces.
 

Fradays 1st law of electr­olysis

Faraday's first law of electr­olysis states that the amount of reaction that occurs at any electrode during electr­olysis by a current is directly propor­tional to the quantity of electric current passed through the electr­olyte
Mathem­ati­cally
M∝Q
M=zQ
But, Q=IT
So, M=ZIT
Where:
z = electr­och­emical equivalent {96500}

Product Formation

This involves the reaction which takes place between the anode and cathode.
M=ZIT -- (i)
M=RAM x IT/f --(ii)
M=MF/f x IT -- (iii)
V/MV = IT/f -- (iv)
Note that:
' / ' means division
 

Faradays 2nd law of electr­olysis

The masses of different ions liberated at the electrodes when the same amount of electr­icity is passed through different electr­olytes is directly propor­tional to their chemical equiva­lents
Mathem­ati­cally
n∝1/e
n=k/e
k=ne
So, ne(1)=­ne(2)

Cost of electr­icity

Q1/Q2 = C1/C2
Where:
C=cost of electr­icity
Q=quantity of electr­icity
 

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