Corrosion (presentation)

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Reactions At the Anode: Fe Fe ++ + 2e - At the Cathode: 2e - + 2H + H2 (bubbles) In the Electrolyte: H2O OH - + H + Galvanic Cell H2 Bubbles CATHODE (Cu) ELECTROLYTE (H2O + NaCl) Fe ++ + 2 OH - Fe (OH)2 (corrosion product) - e - e Fe ++ ions - e ANODE (Fe) <strong>Corrosion</strong> Product
Cathodic Protection • Each metal has a different potential to donate electrons • Anode always corrodes • To protect a metal – Select a metal that more easily donates electrons – Build a cell with metal to be protected as cathode
Page 1 and 2: Corrosion
Page 3 and 4: Uniform Corrosion • Can be a good
Page 5: Galvanic Corrosion • Chemical rea
Page 9 and 10: Pitting and Crevice Corrosion Elect
Page 11 and 12: Erosion Corrosion • Flow removes
Page 13 and 14: Microbiologically Induced • Bacte
Page 15 and 16: SOLUBILITY OF Fe 3O 4 (µg Fe/kg H
Page 17 and 18: Dissolved Oxygen HTS • Oxygen is
Page 19 and 20: pH Secondary Side • pH controlled
Page 21 and 22: Conductivity Secondary Side • Con
Page 23 and 24: Moderator Over Poisoned • pH 4-6
Page 25 and 26: Flakes Sludge and Scale Scale Boile

Corrosion (presentation)

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