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*Outline*
>Definition
>Electrolyte
>Electrode
>Anode & Cathode
>Formulas
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. |
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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
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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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