![]() The stronger the electromotive force, the more spontaneous the reaction. When redox reactions occur, the electrons experience an electromotive force, a force pushing electrons from a reducing agent to an oxidizing agent. (Note that we multiplied the second reaction by 2 to balance the electrons!) We can write the above reaction in terms of an oxidation and reduction half-reaction that add together to form the overall reaction:Ĭopper is oxidized to form Cu2+: Cu → Cu2+ + 2e-Īg+ is reduced to form Ag: 2Ag+ + 2e- → 2Ag Electrons were transferred from copper to silver. Therefore, copper was oxidized, and silver was reduced. Silver starts with an oxidation number of +1 and ends with an oxidation number of 0. We see that copper begins at an oxidation number of 0 and ends with an oxidation number of +2. The language of reducing and oxidizing agents is not specifically referenced on the exam, but it is helpful to know in developing a conceptual understanding of the chemistry occurring.Īn example of a redox reaction is 2AgNO3 + Cu → Cu(NO3)2 + 2Ag. A good acronym to remember this concept is OIL RIG (oxidation is loss reduction is gain). The reducing agent is oxidized (loses electrons), and the oxidizing agent is reduced (gains electrons). A redox reaction, also known as an oxidation-reduction reaction, is a reaction in which electrons transfer from a reducing agent to an oxidizing agent. We will also look at how electrical power can make nonspontaneous redox reactions occur.īefore jumping into the thermodynamics of electrochemistry, we need to review redox reactions from Unit 4. Then, we can connect that voltage to spontaneity and equilibrium. To understand electrochemistry and its applications, we will examine cell potentials, which are a measure of the voltage released during redox reactions. However, another aspect of energy we have yet to discuss is electricity!Įlectrochemistry is the study of redox reactions and how we can use redox reactions to produce electrical energy. Throughout this unit, we centered most of our discussion around the topics of entropy and Gibbs Free Energy.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |