ELC_Electrochemistry Module Overview

Electrochemistry Module Overview

Introduction

In this module you will learn more about oxidation-reductions. You will learn how to balance these reactions and to perform stoichiometric calculations on these specific reactions. You will also learn about different examples of oxidation reactions and their impact on our lives. You will also explore electrolysis, galvanic cells, reduction potentials, and free energy.

Module Lessons Preview

• How are oxidation numbers assigned to each atom in a formula?
• How are equations balanced in acidic or basic solution using the ion-electron method?
• How are stoichiometric calculations performed for redox reactions?
• What is a galvanic cell?
• What is an anode and cathode? How are standard reduction potentials utilized in determining cell potential for a given reaction?
• What makes a spontaneous redox cell?
• How is free energy change calculated for a reaction from its cell potential?
• What is electrolysis?
• How are stoichiometric calculations performed for electrolysis?

Key Terms

• Anode - The positive electrode in a gas discharge tube. The electrode at which oxidation occurs during an electrochemical change
• Cathode - The negative electrode in a gas discharge tube. The electrode at which reduction occurs during an electrochemical change.
• Cell Reaction - The overall chemical change that takes place in an electrolytic cell or a galvanic cell.
• Galvanic Cell - An electrochemical cell in which a spontaneous redox reaction produces electricity.
• Half-cells - That part of a galvanic cell in which either oxidation or reduction takes place.
• Salt-Bridge - A tube that contains an electrolyte that connects the two half-cells of a galvanic cell.
• Reduction Potential - A measure of the tendency of a chemical species to acquire electrons and thereby be reduced.
• Standard Reduction Potential - The reduction potential of a half-reaction at 25 °C when all ion concentrations are 1 M and the partial pressures of all gases are 1 atm.
• Cell Potential, E_cell - The overall chemical change that takes place in an electrolytic cell or a galvanic cell.
• Standard Cell Potential, E°_cell - The potential of a galvanic cell at 25 °C and when all ion concentrations are exactly 1 M and the partial pressures of all gases are 1 atm.
• Faraday (F) - One mole of electrons; 9.65 x 10⁴coulombs
• Electrolysis - the production of a chemical change by the passage of electricity through a solution that contains ions or through a molten ionic compound
• Electrolysis Cell - an apparatus for electrolysis
• Ampere (A) - The SI unit for electric current; one coulomb per second
• Coulomb (C) - The SI unit of electrical charge; the charge on 6.25 x 10¹⁸ electrons; the amount of charge that passes a fixed point of a wire conductor when a current of 1 A flows for 1 s.

eTextbook Reminder

As you read these content pages, also read the corresponding content in your etextbook. Work the example problems in the text as you read to make sure that you understand. The etextbook sections will be listed with the corresponding content pages on your schedule.  

Electrochemistry Practice Problems

Before you begin, print the module practice problems found below.  You should complete a section of problems after covering that particular portion of the content. 

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