An alloy corrodes in the active state in an acidic solution in the presence of the...
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An alloy corrodes in the active state in an acidic solution in the presence of the redox couple Fe/Fe+. The corrosion potential and corrosion current are -0.35 V vs. SHE and 10 A/cm. Given the following, calculate the concentration of Fe* oxidizer. Recalculate the oxidizer concentration for an exchange current density of 0.1 and 1 A/cm for the redox couple. (10 marks) Given: The reduction is under activation control with b. = -0.1 V/decade, Concentration of Fe+ = 106 M The exchange current density of Fe3+ / Fe+ = 0.01 A/cm, Assume that reduction of Fe3+ to Fe2+ is the primary reduction reaction causing corrosion of the metal. An alloy corrodes in the active state in an acidic solution in the presence of the redox couple Fe/Fe+. The corrosion potential and corrosion current are -0.35 V vs. SHE and 10 A/cm. Given the following, calculate the concentration of Fe* oxidizer. Recalculate the oxidizer concentration for an exchange current density of 0.1 and 1 A/cm for the redox couple. (10 marks) Given: The reduction is under activation control with b. = -0.1 V/decade, Concentration of Fe+ = 106 M The exchange current density of Fe3+ / Fe+ = 0.01 A/cm, Assume that reduction of Fe3+ to Fe2+ is the primary reduction reaction causing corrosion of the metal.
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