/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 105 If you were going to apply a sma... [FREE SOLUTION] | 91影视

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Chapter 20: Problem 105

If you were going to apply a small potential to a steel ship resting in the water as a means of inhibiting corrosion, would you apply a negative or a positive charge? Explain.

Short Answer

Expert verified
To inhibit corrosion on a steel ship resting in water, a negative charge should be applied. This makes the steel ship act as a cathode, suppressing the oxidation (anodic) reaction that leads to corrosion. By applying a negative charge, we effectively utilize the principle of cathodic protection to prevent the metal surface from corroding.

Step by step solution

01

Identify the electrode reactions involved in corrosion

The primary reactions in the corrosion process are anodic and cathodic half-cell reactions. At the anode, metal atoms are oxidized to form metal ions that dissolve in the environment. At the cathode, reduction occurs, which can involve different reactants such as oxygen. The overall corrosion process involves the transfer of electrons from the anode to the cathode through the metal.
02

Recognize the principle of cathodic protection

Cathodic protection is a technique used to prevent corrosion of a metal surface (like a steel ship in water) by making the metal surface act as a cathode and avoiding the anodic reaction (which leads to corrosion). This can be achieved by applying an external current or by connecting the protected metal to a more reactive (easily-corroded) metal called the sacrificial anode.
03

Determine the type of charge that should be applied

The goal is to ensure that the steel ship acts as a cathode, which means that we want to suppress the oxidation (anodic) reaction that leads to corrosion. Hence, we should apply a negative charge to the steel ship, since this charge will force the metal to act as a cathode and inhibit any further corrosion.
04

Conclusion

To inhibit corrosion on a steel ship resting in water, a negative charge should be applied. This will ensure that the steel ship acts as a cathode, suppressing the oxidation reaction that leads to corrosion.

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Most popular questions from this chapter

(a) \(\mathrm{A} \mathrm{Cr}^{3+}(a q)\) solution is electrolyzed, using a current of \(7.60 \mathrm{~A}\). What mass of \(\mathrm{Cr}(s)\) is plated out after \(2.00\) days? (b) What amperage is required to plate out \(0.250 \mathrm{~mol} \mathrm{Cr}\) from a \(\mathrm{Cr}^{3+}\) solution in a period of \(8.00 \mathrm{~h}\) ?

(a) Write the reactions for the discharge and charge of a nickel-cadmium rechargeable battery. (b) Given the following reduction potentials, calculate the standard emf of the cell: $$ \begin{array}{r} \mathrm{Cd}(\mathrm{OH})_{2}(s)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Cd}(s)+2 \mathrm{OH}^{-}(a q) \\ \mathrm{NiO}(\mathrm{OH})(s)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{e}^{-} \longrightarrow \mathrm{Ni}(\mathrm{OH})_{2}(s)+\mathrm{OH}^{-}(a q) \\ E_{\mathrm{red}}^{\circ}=+0.49 \mathrm{~V} \end{array} $$ (c) A typical nicad voltaic cell generates an emf of \(+1.30 \mathrm{~V}\). Why is there a difference between this value and the one you calculated in part (b)? (d) Calculate the equilibrium constant for the overall nicad reaction based on this typical emf value.

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The \(K_{\infty}\) value for \(\mathrm{PbS}(s)\) is \(8.0 \times 10^{-28} .\) By using this value together with an electrode potential from Appendix \(\mathrm{E}\), determine the value of the standard reduction potential for the reaction $$ \mathrm{PbS}(s)+2 \mathrm{e}^{-}-\cdots \mathrm{Pb}(s)+\mathrm{S}^{2-}(a q) $$

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