Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 17: Problem 27

Describe a galvanic cell, and give an example.

Short Answer

Expert verified
A galvanic cell is a device that converts chemical energy into electrical energy through a spontaneous redox reaction. It is composed of two half cells, each containing an electrode and an electrolyte. The Daniel cell, composed of a copper electrode in a copper sulphate solution and a zinc electrode in a zinc sulphate solution, is an example of a galvanic cell.

Step by step solution

01

Description of a Galvanic Cell

A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction. It consists of two half-cells. Each half-cell represents a certain reaction involving a particular metal and its ion. Each half-cell contains an electrode (metal strip) and an electrolyte (solution).
02

Function of a Galvanic Cell

In a galvanic cell, the redox reaction is split into two half-reactions, oxidation and reduction, which occur in separate half-cells. The electrode where oxidation takes place is called the anode, while the electrode where reduction occurs is called the cathode. Electrons move from anode (where oxidation occurs) to the cathode (where reduction occurs) through an external wire, creating an electric current.
03

Example of a Galvanic Cell

An example of a galvanic cell is the Daniel cell. It has a copper electrode immersed in a copper sulphate solution which creates the reduction half-cell, and a zinc electrode immersed in a zinc sulphate solution which creates the oxidation half-cell. In this cell, zinc is oxidized (loses electrons) and copper ion in the solution is reduced (gains electrons). The resulting electric current is then able to do work.

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

Describe the components of an electro- chemical cell.

Define electrochemistry.

In an electrochemical cell, what role does the porous barrier play? What would happen without it?

What name is given to an electrode at which oxidation occurs? at which reduction occurs?

Calculate the Equilibrium Constant, using the Standard Cell Voltage The graphing calculator can run a program that calculates the equilibrium constant for an electrochemical cell using an equation called the Nernst equation, given the standard potential and the number of electrons transferred. Given that the standard potential is 2.041 V and that two electrons are transferred, you will calculate the equilibrium constant. The program will be used to make the calculations. Go to Appendix c. If you are using a TI-83 Plus, you can download the program NERNST and data and run the application as directed. If you are using another calculator, your teacher will provide you with key- strokes and data sets to use. After you have run the program, answer the following questions. \begin{equation} \begin{array}{l}{\text { a. What is the equilibrium constant when }} \\\ {\text { the standard potential is } 0.099 ?} \\ {\text { b. What is the equilibrium constant when }} \\ {\text { the standard potential is } 1.125 ?} \\\ {\text { c. What is the equilibrium constant when }} \\ {\text { the standard potential is } 2.500 ?}\end{array} \end{equation}
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

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