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Chapter 17: Q46E (page 961)

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?

Short Answer

Expert verified

When \(B\) and \(C\) come into contact,\(B\) will corrode and \(C\) will not.

Step by step solution

01

Metal corrosion:

  • Metal corrodes when it interacts with another material, such as oxygen, hydrogen, an electrical current, or even dirt and germs.
  • Corrosion can also occur when metals such assteel are subjected to excessive tension, causing the substance to split.
02

Find the metal corrodes:

  • Since\(B\)corrodes when\(A\)and\(B\)comes into contact and\(A\)does not, it means that\(B\)is more likely to corrode because it has a lower reduction potential.
  • And because\(A\)corrodes when\(A\)and\(C\)comes into contact and\(C\)does not,\(A\)has a lower reduction potential than\(C\).
  • So\(C\)has the highest reduction potential,\(B\)the lowest and\(A\)is in between the two.
  • Once we know that, it is easy to conclude that when \(B\) and \(C\) come into contact, \(B\) will corrode and \(C\) will not.

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Most popular questions from this chapter

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.

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

For the scenario in the previous question, how many electrons moved through the circuit.

From the information provided, use cell notation to describe the following systems:

(a) In one half-cell, a solution of \({\rm{Pt}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}\)forms Pt metal, while in the other half-cell, Cu metal goes into a \({\rm{Cu}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}\)solution with all solute concentrations 1M.

(b) The cathode consists of a gold electrode in a \(0.55{\rm{MAu}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_3}\) solution and the anode is a magnesium electrode in \(0.75{\rm{MMg}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}\) solution.

(c) One half-cell consists of a silver electrode in a \(1{\rm{MAgN}}{{\rm{O}}_3}\) solution, and in the other half-cell, a copper electrode in \(1M{\rm{Cu}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}\) is oxidized.

For each of the following balanced half-reactions, determine whether an oxidation or reduction is occurring.

(a) \({\bf{C}}{{\bf{l}}^{\bf{ - }}}{\bf{ + 3}}{{\bf{e}}^{\bf{ - }}} \to {\bf{C}}{{\bf{l}}_{\bf{2}}}\)

(b) \({\bf{M}}{{\bf{n}}^{{\bf{2 + }}}} \to {\bf{Mn}}{{\bf{O}}_{\bf{2}}}\)

(c) \({{\bf{H}}_{\bf{2}}} \to {{\bf{H}}^{\bf{ + }}}\)

(d) \({\bf{NO}}_{\bf{3}}^{\bf{ - }} \to {\bf{NO}}\)

What mass of zinc is required to galvanize the top of a 3.00 m × 5.50 m sheet of iron to a thickness of0.100 mm of zinc? If the zinc comes from a solution of \(Zn{\left( {N{O_3}} \right)_2}\) and the current is 25.5 A, how long will it take to galvanize the top of the iron? The density of zinc is 7.140 g/cm3
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