title: Half-cell
text: # Half-cell
  
  In electrochemistry, a half-cell is a structure that contains a conductive electrode and a surrounding conductive electrolyte separated by a naturally occurring Helmholtz double layer. Chemical reactions within this layer momentarily pump electric charges between the electrode and the electrolyte, resulting in a potential difference between the electrode and the electrolyte. The typical anode reaction involves a metal atom in the electrode being dissolved and transported as a positive ion across the double layer, causing the electrolyte to acquire a net positive charge while the electrode acquires a net negative charge. The growing potential difference creates an intense electric field within the double layer, and the potential rises in value until the field halts the net charge-pumping reactions. This self-limiting action occurs almost instantly in an isolated half-cell; in applications two dissimilar half-cells are appropriately connected to constitute a Galvanic cell.
  
  A standard half-cell consists of a metal electrode in a 1 molar (1 mol/L) aqueous solution of the metal's salt, at 298 kelvins (25 °C). The electrochemical series, which consists of standard electrode potentials and is closely related to the reactivity series, was generated by measuring the difference in potential between the metal half-cell in a circuit with a standard hydrogen half-cell, connected by a salt bridge.
  
  The standard hydrogen half-cell:
  
      $2H^+(aq)$ + $2e^−$ → $H_2(g)$
  
  The half-cells of a Daniell cell:
  
      Original equation
         Zn + $Cu^{2+}$ → $Zn^{2+}$ + Cu
      Half-cell (anode) of Zn
         Zn → $Zn^{2+}$ + $2e^−$
      Half-cell (cathode) of Cu
         $Cu^{2+}$ + $2e^−$ → Cu
  