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Chapter 18: Problem 122

Which of the following statements concerning corrosion is(are) true? For the false statements, correct them. a. Corrosion is an example of an electrolytic process. b. Corrosion of steel involves the reduction of iron coupled with the oxidation of oxygen. c. Steel rusts more easily in the dry (arid) Southwest states than in the humid Midwest states. d. Salting roads in the winter has the added benefit of hindering the corrosion of steel. e. The key to cathodic protection is to connect via a wire a metal more easily oxidized than iron to the steel surface to be protected.

Short Answer

Expert verified
a. False - Corrosion is an example of an electrochemical process, not an electrolytic process. b. True - Corrosion of steel involves the reduction of iron coupled with the oxidation of oxygen. c. False - Steel rusts more easily in humid environments, like the Midwest states. d. False - Salting roads in the winter actually accelerates the corrosion of steel. e. True - The key to cathodic protection is to connect via a wire a metal more easily oxidized than iron to the steel surface to be protected.

Step by step solution

01

Statement a

Corrosion is an example of an electrolytic process. False. Corrosion is an example of an electrochemical process, not an electrolytic process. In electrolytic processes, an external potential is applied to force a non-spontaneous reaction. In corrosion, reactions occur spontaneously without any external potential.
02

Statement b

Corrosion of steel involves the reduction of iron coupled with the oxidation of oxygen. True. The corrosion of steel occurs when the iron in steel reacts with oxygen and water in the environment, forming hydrated iron(III) oxide (rust). In this process, iron gets oxidized, and oxygen gets reduced.
03

Statement c

Steel rusts more easily in the dry (arid) Southwest states than in the humid Midwest states. False. Steel rusts more easily in humid environments, like the Midwest states, where there is more moisture and oxygen available for the corrosion process. In the dry Southwest states, the arid conditions lead to slower rates of corrosion.
04

Statement d

Salting roads in the winter has the added benefit of hindering the corrosion of steel. False. Salting roads in the winter actually accelerates the corrosion of steel. The added salt increases the conductivity of water, enabling the corrosion process to occur at a faster pace.
05

Statement e

The key to cathodic protection is to connect via a wire a metal more easily oxidized than iron to the steel surface to be protected. True. Cathodic protection works by connecting a more easily oxidized metal, known as a sacrificial anode, to the steel surface. This sacrificial anode gets oxidized preferentially, protecting the steel from corrosion and acting as a barrier.

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Most popular questions from this chapter

Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are \(1.0 M\) and that all partial pressures are \(1.0 \mathrm{~atm}\).

A galvanic cell is based on the following half-reactions: $$ \begin{aligned} \mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Fe}(s) & \mathscr{E}^{\circ} &=-0.440 \mathrm{~V} \\ 2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{H}_{2}(g) & \mathscr{E}^{\circ} &=0.000 \mathrm{~V} \end{aligned} $$ where the iron compartment contains an iron electrode and \(\left[\mathrm{Fe}^{2+}\right]=1.00 \times 10^{-3} M\) and the hydrogen compartmentcontains a platinum electrode, \(P_{\mathrm{H}_{2}}=1.00 \mathrm{~atm}\), and a weak acid, HA, at an initial concentration of \(1.00 M .\) If the observed cell potential is \(0.333 \mathrm{~V}\) at \(25^{\circ} \mathrm{C}\), calculate the \(K_{\mathrm{a}}\) value for the weak acid HA.

The compound with the formula \(\mathrm{TII}_{3}\) is a black solid. Given the following standard reduction potentials, $$ \begin{aligned} \mathrm{Tl}^{3+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Tl}^{+} & \mathscr{E}^{\circ}=1.25 \mathrm{~V} \\ \mathrm{I}_{3}^{-}+2 \mathrm{e}^{-} \longrightarrow 3 \mathrm{I}^{-} & \mathscr{E}^{\circ}=0.55 \mathrm{~V} \end{aligned} $$ would you formulate this compound as thallium(III) iodide or thallium(I) triiodide?

Three electrochemical cells were connected in series so that the same quantity of electrical current passes through all three cells. In the first cell, \(1.15 \mathrm{~g}\) chromium metal was deposited from achromium(III) nitrate solution. In the second cell, \(3.15 \mathrm{~g}\) osmium was deposited from a solution made of \(\mathrm{Os}^{n+}\) and nitrate ions. What is the name of the salt? In the third cell, the electrical charge passed through a solution containing \(\mathrm{X}^{2+}\) ions caused deposition of \(2.11 \mathrm{~g}\) metallic \(\mathrm{X}\). What is the electron configuration of \(\mathrm{X}\) ?

Consider the galvanic cell based on the following halfreactions: $$ \begin{array}{ll} \mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn} & \mathscr{E}^{\circ}=-0.76 \mathrm{~V} \\ \mathrm{Fe}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Fe} & \mathscr{E}^{\circ}=-0.44 \mathrm{~V} \end{array} $$ a. Determine the overall cell reaction and calculate \(\mathscr{E}_{\text {cell }}^{\circ}\) b. Calculate \(\Delta G^{\circ}\) and \(K\) for the cell reaction at \(25^{\circ} \mathrm{C}\). c. Calculate \(\mathscr{E}_{\text {cell }}\) at \(25^{\circ} \mathrm{C}\) when \(\left[\mathrm{Zn}^{2+}\right]=0.10 M\) and \(\left[\mathrm{Fe}^{2+}\right]=1.0 \times 10^{-5} M\)
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