Electrochemistry
ElectrochemistryChemical reactions at an electrode, galvanic and electrolytic cellsA Chem1 Reference TextStephen K. Lower Simon Fraser University1Table of contents1:Chemistry and electricity . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3Electroneutrality . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3Potential differences at interfaces . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 52:Electrochemical cells.
the concentration of Zn2+ is still too low (around 10–10 M) to be detected by ordinary chemi-cal means. Fig. 1: Oxidation of metallic zinc in contact with water. Page 4 Electrochemistry There would be no build-up of opposing charges in the two phases if the excess electrons
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