Class 12 Chemistry Electrochemistry Standard hydrogen electrode

Standard hydrogen electrode

  • The electrode is connected to a standard hydrogen electrode (SHE) to constitute a cell
  • It consists of a platinum electrodecoated with a layer of platinum black.

  • The electrode is immersed in an acidicsolution and the pure hydrogen gas is bubbled through it.
  • Theconcentration of the reduced form and the oxidized form of hydrogen issustained at unity with following conditions:
  • Pressure of hydrogen gas = 1 bar
  • Concentration of hydrogen ion in the solution = 1 molar

Ecell = Ecathode – Eanode

Ecell = Ecathode – 0 = Ecathode

  • The measured Emf of the cell:

Pt| H2 (1 bar)| H+ (1M) || Cu2+ (1M)| Cu is 0.34 V.

The positive value of the standard electrode potential signifies the easy reduction of Cu2+ ions than H+ ions.

  • The measured Emf of the cell

Pt| H2 (1 bar)| H+ (1M) || Zn2+ (1M)| Zn is -0.76 V.

The negative value of the standard electrode potential signifies that the hydrogen ions oxidizes the zinc (or it can be said that zinc can reduce hydrogen ions).

  • An electrode with standard electrode potential greater than zero is stable in its reduced form compared tohydrogen gas.
  • Whereas an electrode with negative standard electrode potential is less stable in its reduced form compared to hydrogen gas.
  • This decreases the standard electrodepotential which in turn decreases the oxidizing power ofthe specific electrode on the left and increases the reducing power of the electrodeto the right of the reaction.

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