Transcription of Electrochemistry
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Electrochemistry
ElectrochemistryChemical reactions at an electrode, galvanic and electrolytic cellsA Chem1 Reference TextStephen K. Lower Simon Fraser University1 Table of contents1:Chemistry and electricity .. 3 Electroneutrality .. 3 Potential differences at interfaces .. 52:Electrochemical cells .. 6 Transport of charge within the cell .. 7 Cell description conventions .. 8 Electrodes and electrode reactions .. 8 Standard half-cell potentials .. 9 Reference electrodes .. 113:Prediction and significance of cell potentials .. 12 Cell potentials and the electromotive series .. 13 Cell potentials and free energy .. 134:The Nernst equation .. 18 Concentration cells .. 23 Thermodynamics of galvanic cells .. 23 Analytical applications of the Nernst equation .. 23 Membrane potentials.
Sep 23, 2004 · 1.1 Electroneutrality Nature seems to strongly discourage any process that would lead to an excess of positive or negative charge in matter. Suppose, for example, that we immerse a piece of zinc metal in pure water. A small number of zinc atoms go into solution as Zn ions, leaving their electrons behind in the metal: Zn(s) → Zn 2+ + 2 e–
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