Electrolytic Cells and Galvanic/Voltaic Cells
Discover how electrolytic cells and galvanic/voltaic cells utilize electrical energy to create chemical energy. Understand the differences between spontaneous and non-spontaneous reactions in these cells, and learn about the two types of electrolytic cells - fused salt cells and electroplating cells. Explore the process of electroplating and the importance of electrode polarity in these cells.
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Presentation Transcript
Electrolytic Cells utilizes electrical energy to create chemical energy
galvanic/Voltaic cell chemical potential energy electrical potential energy electrolytic cell (battery needed) chemical rxns can produce electricity in galvanic/Voltaic cells (spontaneous rxn - exothermic) OR electrical energy used to carry out chemical reactions in electrolytic cell (non-spont rxn - endothermic)
spontaneous reactions: (galvanic/Voltaic cell) non-spontaneous reactions: (electrolytic cell) e- flow: (-) ANODE to (+) CATHODE generates own power produces energy exo anode: higher metal on table J cathode: lower metal on table J e- flow: (+) ANODE to (-) CATHODE needs power source: battery consumes energy endo anode: lower metal on table J cathode: higher metal on table J
two types of electrolytic cells 1. fused salt cells used to purify metals (fused means melted!) 2. electroplating cells designed to cover a surface with metal so will have specific properties
Electroplating electroplating: putting one metal on top of another (anode) onto object (cathode) to be plated solution contains ions (Cu+2) of element (Cu) to be plated move desired coating
An Ox ate a Red Cat anode: electrode at which oxidation occurs cathode: electrode at which reduction occurs electrode polarity opposite than galvanic cell! anode is POSITIVE cathode is NEGATIVE
A POX on Electrolytic Cells Anode Positive Oxidation electrolytic cell: polarity determined by outside power supply anode is attached to (+) terminal cathode is attached to (-) terminal
Can Cu be plated onto Al? Al above Cu in Table J reaction will nothappen spontaneously so external energy source (power supply or battery) needed to force reaction to occur (plating Cu on Al) cathode (-): object to be plated (must be more reactive than anode higher on table J) anode (+): made of metal want to plate on object (must be less reactive than cathode lower on table J) solution: contains ions of metal to be plated (anode)
(+) (-) Battery anode: where oxidation happens (+) Cu Cu+2 + 2e- (-) cathode: obj being plated (Al) - where reduction happens Cu(s) Cu+2 Cu+2 + 2e- Cu SO4-2 Note: just moving Cu around
In summation: electrolytic cells: galvanic or Voltaic cells: use spontaneous SR rxn to produce flow of electrons (electricity) use flow of electrons (electricity) to force non-spontaneous rxn to occur endothermic electrons flow from anode (oxidized substance) to cathode (reduced substance) exothermic electrons flow from anode (oxidized substance) to cathode (reduced substance)
