/*! 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 22 Define electrolysis and relate t... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 20: Problem 22

Define electrolysis and relate the definition to the spontaneity of redox reactions.

Short Answer

Expert verified
Electrolysis is a process to drive non-spontaneous redox reactions using electricity.

Step by step solution

01

Understand Electrolysis

Electrolysis is a chemical process that uses an electric current to drive a non-spontaneous chemical reaction. This process requires an external power source to supply the necessary energy for the reaction to occur.
02

Define Redox Reactions

Redox reactions involve the transfer of electrons between two species. In these reactions, one substance is oxidized (loses electrons), and another is reduced (gains electrons).
03

Relate to Non-Spontaneity

In electrolysis, the redox reactions involved are non-spontaneous, meaning they do not occur on their own and need an electrical input to proceed. This is because the energy to perform the reaction is greater than what's available from the natural environment, so an external power source is required to force the reaction to take place.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Redox Reactions
Redox reactions, short for reduction-oxidation reactions, are fundamental chemical processes. They are characterized by the movement of electrons between distinct molecules or atoms.
In any redox reaction, one species donates electrons and gets oxidized, while another accepts electrons and gets reduced.

To recognize a redox reaction, look for:
  • Changes in oxidation numbers: The element being oxidized increases its oxidation state, while the one being reduced decreases its oxidation state.
  • Electron transfer: Reactions where electrons move from one atom or molecule to another.
  • Energy changes: Often redox reactions involve changes in energy, either releasing energy (exothermic) or requiring energy (endothermic).
These reactions are crucial in numerous natural and man-made processes, including cellular respiration and battery operation.
Non-Spontaneous Reactions
Non-spontaneous reactions do not naturally occur without external intervention. They require an input of energy to initiate. One common method of inducing non-spontaneous reactions is through electrolysis.
Essentially, these reactions need a catalyst to overcome the energy barrier that prevents them from happening on their own.

In electrolysis:
  • An external power source provides the necessary energy to start and sustain the reaction.
  • These processes are typically endothermic with energy input often coming from electricity.
  • Energy sources overcome the reaction's natural tendency to remain stagnant or unchanged.
Think of non-spontaneous reactions like a ball on a hill that needs an extra push to start rolling down; this is the push electrolysis provides in chemical scenarios.
Oxidation and Reduction
Oxidation and reduction are two halves of a redox reaction, intimately connected in every process where electron exchange occurs.
Oxidation describes when a molecule, atom, or ion loses one or more electrons. Conversely, reduction refers to the gain of electrons by a molecule, atom, or ion.

Features of oxidation include:
  • Increase in oxidation state.
  • Loss of electrons, often making the substance more positive.
Meanwhile, reduction involves:
  • Decrease in oxidation state.
  • Gain of electrons, often leading to a more negative charge.
Understanding these processes is crucial, as they occur in many vital biological and chemical activities, from how our bodies utilize oxygen to how metal ores are refined in industrial settings.

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

Explain why lithium is a good choice for the anode of a battery.

If the volume of a sample of chlorine gas is 8.2 \(\mathrm{L}\) at 1.2 atm and 306 \(\mathrm{K}\) , what volume will the gas occupy at STP? (Chapter 13\()\)

Electroplating Figure 20.27 shows a key being electroplated with copper in an electrolytic cell. Where does oxidation occur? Explain your answer.

Write the balanced chemical equation for the standard cell notations listed below. $$ \begin{array}{l}{\text { a. } \mathrm{I}^{-}\left|\mathrm{I}_{2} \| \mathrm{Fe}^{3+}\right| \mathrm{Fe}^{2+}} \\ {\text { b. } \mathrm{Sn}\left|\mathrm{Sn}^{2+} \| \mathrm{Ag}^{+}\right| \mathrm{Ag}} \\\ {\text { c. } \mathrm{Zn}\left|\mathrm{Zn}^{2+} \| \mathrm{Cd}^{2+}\right| \mathrm{Cd}}\end{array} $$

Hypothesize The potential of a half-cell varies with concentration of reactants and products. For this reason, standard potentials are measured at 1\(M\) concentration. Maintaining a pressure of 1 atm is especially important in half-cells that involve gases as reactants or products. Suggest a reason why gas pressure is critical in these cells.
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

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.