Log out Go to App
Go to App

Learning Materials

Features

Discover

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

Expert verified
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).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Why does chromium in stainless steels make them more corrosion resistant in many environments than plain carbon steels? Forms of Corrosion

A piece of corroded steel plate was found in a submerged ocean vessel. It was estimated that the original area of the plate was 10 in. \(^{2}\) and that approximately \(2.6 \mathrm{~kg}\) had corroded away during the submersion. Assuming a corrosion penetration rate of \(200 \mathrm{mpy}\) for this alloy in seawater, estimate the time of submersion in years. The density of steel is \(7.9 \mathrm{~g} / \mathrm{cm}^{3}\)

Briefly describe the two techniques that are used for galvanic protection. Oxidation.

For each of the metals listed in the following table, compute the Pilling- Bedworth ratio. Also, on the basis of this value, specify whether you would expect the oxide scale that forms on the surface to be protective, and then justify your decision. Density data for both the metal and its oxide are also tabulated. \begin{tabular}{lccc} \hline & Metal Metal & Density \(\left(\mathrm{g} / \mathrm{cm}^{3}\right)\) & Metal Oxide & Oxide Density \(\left(\mathrm{g} / \mathrm{cm}^{\mathbf{7}}\right)\) \\ \hline \(\mathrm{Zr}\) & \(6.51\) & \(\mathrm{ZrO}_{2}\) & \(5.89\) \\ \(\mathrm{Sn}\) & \(7.30\) & \(\mathrm{SnO}_{2}\) & \(6.95\) \\ \(\mathrm{Bi}\) & \(9.80\) & \(\mathrm{Bi}_{2} \mathrm{O}_{3}\) & \(8.90\) \\ \hline \end{tabular}

Briefly explain why cold-worked metals are more susceptible to corrosion than noncoldworked metals.
See all solutions

Recommended explanations on Physics Textbooks

Fundamentals of Physics

Read Explanation

Quantum Physics

Read Explanation

Physics of Motion

Read Explanation

Energy Physics

Read Explanation

Particle Model of Matter

Read Explanation

Further Mechanics and Thermal Physics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free