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Chapter 17: Problem 1

(a) Briefly explain the difference between oxidation and reduction electrochemical reactions. (b) Which reaction occurs at the anode and which at the cathode?

Short Answer

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Question: Explain the difference between oxidation and reduction electrochemical reactions and identify which reaction occurs at the anode and which occurs at the cathode. Answer: Oxidation and reduction electrochemical reactions are two opposite types of reactions that involve the transfer of electrons. In an oxidation reaction, a chemical species loses electrons, and its oxidation state increases. In contrast, a reduction reaction involves a chemical species gaining electrons and decreasing its oxidation state. In an electrochemical cell, the oxidation reaction occurs at the anode, while the reduction reaction takes place at the cathode.

Step by step solution

01

Define Oxidation and Reduction Reactions

Oxidation and reduction reactions are two opposite types of reactions that involve the transfer of electrons. In an oxidation reaction, a chemical species loses electrons, resulting in an increase in its oxidation state. In a reduction reaction, a chemical species gains electrons, leading to a decrease in its oxidation state.
02

Provide Examples of Oxidation and Reduction Reactions

A common example of an oxidation reaction is the reaction of iron with oxygen to form iron oxide (rust): 4Fe (s) + 3O2 (g) -> 2Fe2O3 (s) In this reaction, iron (Fe) loses 3 electrons and gets oxidized, while oxygen (O2) gains 4 electrons and gets reduced. Another example is the reaction between hydrogen and oxygen to form water: 2H2 (g) + O2 (g) -> 2H2O (l) In this reaction, hydrogen (H2) loses 1 electron and gets oxidized, while oxygen (O2) gains 2 electrons and gets reduced.
03

Define Anode and Cathode

The anode and cathode are two electrodes in an electrochemical cell where redox reactions take place. The anode is the electrode where oxidation occurs, and the cathode is the electrode where reduction occurs. Electrons flow from the anode to the cathode in the external circuit.
04

Identify the Reactions at the Anode and the Cathode

In an electrochemical cell, the oxidation reaction occurs at the anode, and the reduction reaction occurs at the cathode. This is because the anode is the electrode where electrons are lost (oxidation), and the cathode is the electrode where electrons are gained (reduction).

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Most popular questions from this chapter

Briefly explain why, for a small anode-tocathode area ratio, the corrosion rate will be higher than for a large ratio.

For the following pairs of alloys that are coupled in seawater, predict the possibility of corrosion; if corrosion is probable, note which metal/alloy will corrode. (a) Aluminum and magnesium (b) Zinc and a low-carbon steel (c) Brass ( \(60 \mathrm{wt} \% \mathrm{Cu}-40 \mathrm{wt} \% \mathrm{Zn}\) ) and Monel \((70 \mathrm{wt} \% \mathrm{Ni}-30 \mathrm{wt} \% \mathrm{Cu})\) (d) Titanium and 304 stainless steel (e) Cast iron and 316 stainless steel

An electrochemical cell is composed of pure copper and pure lead electrodes immersed in solutions of their respective divalent ions. For a \(0.6 M\) concentration of \(\mathrm{Cu}^{2+}\), the lead electrode is oxidized, yielding a cell potential of \(0.507 \mathrm{~V} .\) Calculate the concentration of \(\mathrm{Pb}^{2+}\) ions if the temperature is \(25^{\circ} \mathrm{C}\).

(a) Compute the voltage at \(25^{\circ} \mathrm{C}\) of an electrochemical cell consisting of pure cadmium immersed in a \(2 \times 10^{-3} M\) solution of \(\mathrm{Cd}^{2+}\) ions, and pure iron in a \(0.4 M\) solution of \(\mathrm{Fe}^{2+}\) ions. (b) Write the spontaneous electrochemical reaction.

Using the results of Problem 17.13, compute the corrosion penetration rate, in mpy, for the corrosion of iron in citric acid (to form \(\mathrm{Fe}^{2+}\) ions) if the corrosion current density is \(1.15 \times 10^{-5} \mathrm{~A} / \mathrm{cm}^{2}\)
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