Iron (Fe) metal is corroded in an aerated dilute acid solution with a pH of 7....

 

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Iron (Fe) metal is corroded in an aerated dilute acid solution with a pH of 7. Since the corrosion potential (Ekor) of this corrosion cell is -0.45 Volt (SHE) at pH=7, calculate the cathodic current density required for oxygen reduction using the following? According to your results, explain which cathodic reaction is dominant in the corrosion of iron for this corrosion cell. (Take RT/F= 0.0591) Given: EoFe = -0.44 V (SHE), aFe2+ = 10-6, Tafel constant, b (2.3a) = 0.06 V/decade, io = 10-11 A.cm-2 EoH = 0.00 V (SHE). Tafel constant, b (2.3a) = 0.12 V/decade, io = 10-10 A.cm-2, PH2= 1 atm. Iron (Fe) metal is corroded in an aerated dilute acid solution with a pH of 7. Since the corrosion potential (Ekor) of this corrosion cell is -0.45 Volt (SHE) at pH=7, calculate the cathodic current density required for oxygen reduction using the following? According to your results, explain which cathodic reaction is dominant in the corrosion of iron for this corrosion cell. (Take RT/F= 0.0591) Given: EoFe = -0.44 V (SHE), aFe2+ = 10-6, Tafel constant, b (2.3a) = 0.06 V/decade, io = 10-11 A.cm-2 EoH = 0.00 V (SHE). Tafel constant, b (2.3a) = 0.12 V/decade, io = 10-10 A.cm-2, PH2= 1 atm.

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