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Chapter 17: Q43E (page 961)

Consider the following metals: Ag, Au, \(Mg, Ni,\)\(and\)\(Zn\). Which of these metals could be used as a sacrificial anode in the cathodic protection of an underground steel storage tank? Steel is mostly iron, so use \( - 0.447\;{\rm{V}}\) as the standard reduction potential for steel.

Short Answer

Expert verified

Theoretically, we could use magnesium and zinc as sacrificial electrodes to prevent the steel tank from corroding.

Step by step solution

01

sacrificial anode cathodic protection:

  • Sacrificial anode cathodic protection (SACP) is a kind of cathodic protection in which less noble material functions as a sacrificial anode and is linked to the structure to be protected via metallic conductors.
  • Magnesium, aluminium, and zinc are the materials employed for this function.
02

Find a sacrificial anode in the cathodic protection:

  • Using metal as a sacrificial anode for a steel tank means that we are using that metal to stop iron in the steel tank from corroding.
  • That means that we have to use a metal that is more likely to corrode than iron, ie. has a lower reduction potential than iron\(( - 0.447\;{\rm{V}})\).
  • We can look up the reduction potentials of each of the metals in the table in the Appendix\(L\)of the book. They are:
  • silver :\(0.7996\;{\rm{V}}\)
  • gold :\(1.692V\)
  • magnesium :\( - 2.372\;{\rm{V}}\)
  • nickel:\( - 0.257\;{\rm{V}}\)
  • zinc:\( - 0.7618\;{\rm{V}}\)
  • Here we can see that the metals that have a lower reduction potential\( - 0.447\;{\rm{V}}\)are magnesium and zinc.
  • Therefore, of the metals in question, theoretically, we could use magnesium and zinc as sacrificial electrodes to prevent the steel tank from corroding but in practice, we would use zinc because magnesium is reactive metal (e.g. magnesium reacts with nitrogen from the air).
  • Magnesium is the most often utilized anode material for exterior protection of underground tanks, and the voltage difference between steel and a magnesium anode is 1.2 to 1.8 V. (depending on the type of magnesium alloy used).

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Most popular questions from this chapter

For each reaction listed, determine its standard cell potential at \({25\circ }{\rm{C}}\) and whether the reaction is spontaneous at standard conditions.

(a)\({\mathop{\rm Mn}\nolimits} (s) + {\rm{N}}{{\rm{i}}^{2 + }}(aq) \to {{\mathop{\rm Mn}\nolimits} ^{2 + }}(aq) + {\rm{Ni}}(s)\)

(b)\(3{\rm{C}}{{\rm{u}}^{2 + }}(aq) + 2{\rm{Al}}(s) \to 2{\rm{A}}{{\rm{l}}^{3 + }}(aq) + 3{\rm{Cu}}(s)\)

(c)\({\rm{Na}}(s) + {\rm{LiN}}{{\rm{O}}_3}(aq) \to {\rm{NaN}}{{\rm{O}}_3}(aq) + {\rm{Li}}(s)\)

(d) \({\rm{Ca}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Ba}}(s) \to {\rm{Ba}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Ca}}(s)\)

If a sample of iron and a sample of zinc come into contact, the zinc corrodes but the iron does not. If a sample of iron comes into contact with a sample of copper, the iron corrodes but the copper does not. Explain this phenomenon.

Suppose you have three different metals, \({\rm{A}}\), \(B\), and \({\rm{C}}\). When metals \({\rm{A}}\) and \(B\) come into contact, \(B\) corrodes and \({\rm{A}}\)do not corrode. When metals \({\rm{A}}\)and \({\rm{C}}\) come into contact, \({\rm{A}}\) corrodes and \({\rm{C}}\) do not corrode. Based on this information, which metal corrodes and which metal does not corrode when \(B\) and \({\rm{C}}\) come into contact?

Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and thereducing agent in each of the reactions of the previous problem.

\(\begin{array}{l}{\bf{(a) H_2O_2 + S}}{{\bf{n}}^{{\bf{2 + }}}} \to {\bf{H_2O + S}}{{\bf{n}}^{{\bf{4 + }}}}\\{\bf{(b) PbO_2 + Hg}} \to {\bf{Hg}}{{\bf{2}}^{{\bf{2 + }}}}{\bf{ + P}}{{\bf{b}}^{{\bf{2 + }}}}\\{\bf{(c) Al + Cr_2O}}{{\bf{7}}^{{\bf{2 - }}}} \to {\bf{A}}{{\bf{l}}^{{\bf{3 + }}}}{\bf{ + C}}{{\bf{r}}^{{\bf{3 + }}}}\end{array}\)

Determine the overall reaction and its standard cell potential at 25 掳C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half-cell consisting of an aluminum electrode

in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?
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