/*! 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 34 Define electrolytic cell, and gi... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Problem 34

Define electrolytic cell, and give an example.

Short Answer

Expert verified
An electrolytic cell drives a non-spontaneous redox reaction through the application of electrical energy, converting electrical into chemical energy. It is composed of two electrodes connected by an external power source, and immersed in an electrolyte. An example is the electrolysis of water, where water is transformed into hydrogen and oxygen gases using electrical energy.

Step by step solution

01

Define Electrolytic Cell

An electrolytic cell is a type of cell that drives a non-spontaneous redox reaction through the application of electrical energy. It's designed to convert electrical energy into chemical energy. Electrolytic cells are composed of two electrodes (anode and cathode) connected by an external power source, and are often immersed in an electrolyte that allows ions to move between the electrodes.
02

Provide an Example of Electrolytic Cell

A common example of an electrolytic cell is the electrolysis of water. In this process, water is transformed into hydrogen and oxygen gases using an electric current. The water acts as an electrolyte, while the two electrodes are often made of inert metals. When electrical energy is applied, water molecules (\(2H_{2}O\)) at the anode get oxidized to form oxygen gas (\(O_{2}\)) and four protons (\(4H^{+}\)). On the other hand, at the cathode, four protons (\(4H^{+}\)) are reduced to form hydrogen gas (\(H_{2}\)). The overall reaction becomes: \(2H_{2}O \rightarrow O_{2} + 2H_{2}\).

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 Reaction
A redox reaction, short for reduction-oxidation reaction, involves the transfer of electrons between two entities. In an electrolytic cell, these reactions are non-spontaneous and require external electrical energy to occur.
  • Reduction is the process in which a molecule, atom, or ion gains electrons, resulting in a decrease in its oxidation state.
  • Oxidation is the opposite process, involving the loss of electrons and an increase in oxidation state.

In an electrolytic cell, the redox reaction is forced to occur under the influence of an external power source. This source provides the electrical energy necessary to drive the reaction forward, forming the basis of processes like electrolysis.
Electrical Energy
Electrical energy plays a crucial role in the functioning of electrolytic cells. It's the driving force that facilitates the transformation of chemical entities by overcoming the energy barrier that prevents spontaneous reactions.

When an external electric current is applied to an electrolytic cell, it flows from an external power source into the system. This current supplies the energy needed for ions to move within the electrolyte and facilitates the redox reactions at the electrodes.
  • Current flows through the circuit, from the positive terminal, through the electrolyte, and back to the negative terminal.
  • The electrons provided by the electrical current enable oxidation at the anode and reduction at the cathode.
Electrolysis
Electrolysis is the process of using electrical energy to produce a chemical change. In the context of an electrolytic cell, it's the method used to decompose compounds into their elemental forms.

Consider the electrolysis of water as an example:
  • The water molecule, acting as an electrolyte, dissociates into ions under the influence of an applied electric current.
  • At the anode, water molecules are oxidized to form oxygen gas. Electrons are released which travel through the external circuit.
  • At the cathode, electrons from the circuit reduce protons to produce hydrogen gas.

This process results in the breakdown of water into hydrogen and oxygen gases, as one of the most well-known applications of electrolysis.
Chemical Energy
Chemical energy in an electrolytic cell is the stored energy within the chemical bonds of the substance undergoing electrolysis. When electrical energy is added to the system, it facilitates chemical reactions that alter these bonds.

During electrolysis, the conversion of electrical energy into chemical energy takes place as new chemical products are formed. This transformation is crucial in applications ranging from water splitting to metal plating, where the chemical energy released during these processes is utilized to achieve desired results.
  • The energy conversion is essential for the production of substances like hydrogen gas in the electrolysis of water.
  • It also has significant industrial uses, such as the electroplating of metals, where metal ions are deposited onto a substrate under applied electric currents.
Electrodes
An electrolytic cell consists of two critical components known as electrodes, termed as the anode and the cathode. These are vital for the process of electrolysis, as they provide the surface on which redox reactions occur.

Electrodes serve different functions in the electrolytic cell:
  • The anode is the electrode where oxidation takes place, losing electrons to the external circuit.
  • The cathode is where reduction occurs, gaining electrons from the external circuit and completing the redox reactions.

Materials for electrodes need to be carefully chosen, often using inert metals like platinum or graphite, especially in simple processes like water electrolysis, to ensure that they do not react with the products or the electrolyte.

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

Determine the oxidation number of each atom in \(\mathrm{CaCO}_{3} .\)

Think of ammonium nitrite as \(\left(\mathrm{NH}_{4}^{+}\right)\left(\mathrm{NO}_{2}^{-}\right)\) and assign oxidation numbers within each ion. Now think of ammonium nitrate as \(\mathrm{N}_{2} \mathrm{H}_{4} \mathrm{O}_{2},\) and assign oxidation numbers. Which assignment makes more sense?

Write the balanced half-reaction for the conversion of \(\mathrm{H}_{2} \mathrm{O}(l)\) to \(\mathrm{O}_{2}(a q)\) in acidic solution.

Discuss methods of reducing corrosion.

Is the reaction below a redox reaction? Explain your answer. $$\mathrm{Ca}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{CaCl}_{2}(s)$$
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

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.