*Outline* >Definition >Electrolyte >Electrode >Anode & Cathode >Formulas
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Electrolysis can be defined as the decomposition of compounds which happens when direct current passes through a solution or molten compound.
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Electrolyte
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This can be defined as a liquid which conduct elections.
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Types of electrolyte
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Strong Electrolyte: These are strong acids and strong bases/alkali's.
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Weak Electrolyte: These are weak acids and weak bases/alkali's.
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Electrode
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This is a metal rod, plate or wire, which conducts electricity in an electrolytic cell.
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Anode: This is the positive electrode through which conventional current enters and electrons leave.
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Cathode: This is the negative electrode through wich conventional current leaves and electrons enter.
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Electrolytic Cell
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This is the setup of two electrodes, placed in an electrolyte, used in the electrolysis of substances.
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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
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Mathematically
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M∝Q
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M=zQ
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But, Q=IT
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So, M=ZIT
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This involves the reaction which takes place between the anode and cathode.
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M=ZIT -- (i)
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M=RAM x IT/f --(ii)
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M=MF/f x IT -- (iii)
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V/MV = IT/f -- (iv)
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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
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Mathematically
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n∝1/e
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n=k/e
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k=ne
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So, ne(1)=ne(2)
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Q1/Q2 = C1/C2
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Where:
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C=cost of electricity
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Q=quantity of electricity
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