Explain why iron nails placed in a solution of FeSO4 inhibit the oxidation of iron (II) to iron...
Question:
Explain why iron nails placed in a solution of FeSO{eq}_4 {/eq} inhibit the oxidation of iron (II) to iron (III).
Oxidation Potential
The redox-half reaction involving the rise in metal ion's oxidation state is known as oxidation. The energy needed in this redox-half reaction is known as the oxidation potential.
Answer and Explanation: 1
The oxidation reaction of iron to {eq}{\rm{F}}{{\rm{e}}^{{\rm{2 + }}}} {/eq} is shown below.
{eq}{\rm{Fe}}\left( {\rm{s}} \right) \to {\rm{F}}{{\rm{e}}^{2 + }}\left( {{\rm{aq}}} \right) + 2{e^ - }\;\;\;\;\;\;{E^{\rm{o}}} = + 0.44\;{\rm{V}} {/eq}
The oxidation reaction of {eq}{\rm{F}}{{\rm{e}}^{{\rm{2}} + }} {/eq} to {eq}{\rm{F}}{{\rm{e}}^{{\rm{3}} + }} {/eq} is shown below.
{eq}{\rm{F}}{{\rm{e}}^{2 + }}\left( {{\rm{aq}}} \right) \to {\rm{F}}{{\rm{e}}^{3 + }}\left( {{\rm{aq}}} \right) + {e^ - }\;\;\;\;\;\;{E^{\rm{o}}} = - 0.77\;{\rm{V}} {/eq}
The oxidation potential of iron to {eq}{\rm{F}}{{\rm{e}}^{{\rm{2}} + }} {/eq} is greater than the oxidation potential of {eq}{\rm{F}}{{\rm{e}}^{{\rm{2}} + }} to {\rm{F}}{{\rm{e}}^{{\rm{3}} + }} {/eq}. Therefore, iron nail placed in a solution of {eq}{\rm{FeS}}{{\rm{O}}_{\rm{4}}} {/eq} inhibit the oxidation of {eq}{\rm{F}}{{\rm{e}}^{{\rm{2}} + }} to {\rm{F}}{{\rm{e}}^{{\rm{3}} + }}. {/eq}
Learn more about this topic:
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Chapter 12 / Lesson 3Cells primarily rely on oxidation and reduction to generate energy. Learn about oxidation and reduction reactions in the body, what oxidative metabolism is, and how energy is produced in the form of ATP.