Explanation
In the electrochemical series,
The more the negative E° value, the more the position of equilibrium lies to the left, then the more readily the metal loses electrons. Hence the more negative E° value, the stronger is the reducing agent.
The more the positive E° value, the more the position of equilibrium lies to the right, then the less readily the metal loses electrons. Hence the more positive E° value, the stronger is the oxidizing agent.
Therefore the order of the reducing power of A, B and C is B > C > A.
Substances with higher reduction potentials are strong oxidizing agents while substances with lower reduction potentials are strong reducing agents. The electrode having higher standard reduction potential acts as cathode and the electrode having lower standard reduction potential acts as anode. If the Ecell value is positive, then the reaction is spontaneous. If the Ecell value is negative, then the reaction is non-spontaneous.
Since, Ecell = Ecathode – Eanode
Therefore, Ecell = Ecathode – Eanode
Ecell = EA – EB = -0.03 - (+0.108) = -0.138 V.
Hence the reaction between A and B is non-spontaneous.
Voltmeter is used to measure the standard electrode potential.
A galvanic cell, or voltaic cell, named after Lugi galvani, or Alessandro volta respectively, is an electrochemical cell that derives electrical energy from spantaneous redox reactions taking place within the cell.
Cathodic Protection is an electrochemical means of corrosion control in which the oxidation reaction in a galvanic cell is concentrated at the anode and suppresses corrosion of the cathode in the same cell. Hence during rusting, oxidation of iron takes place thereby iron acts as anode. So coating iron with metal of lower reduction potential (in comparison to iron) is the best way to prevent its rusting. In this process, the metal with low reduction potential undergoes oxidation (i.e. acts as anode) while iron acts as cathode.
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