L4 - Applications of Spontaneous Redox Reactions

In the previous lesson you saw how an electrolytic cell can be used to produce pure elements such as the gases hydrogen, oxygen, and chlorine, and pure metals like copper. The electrolytic cell causes chemical change by forcing a redox reaction to occur.

In Science 10 you may have seen a demonstration of the reactivity of sodium, potassium, and lithium (group 1 metals) with water. Do you recall which metals reacted most vigorously—so much so that you could see a flame? How could such reactive metals ever be converted into their elemental forms? Is it possible that an electrolytic cell could be used for the production of all metals?

Previously, you observed the operation of laboratory-scale electrolytic cells. How is the electrolytic cell used to plate chromium onto automobile bumpers, as shown in the photograph, similar and different to the cells you build in a laboratory? In this lesson you will investigate society's use of electrolytic cells as a technology.

Consider the following question as you complete this lesson:

• What are some of the practical applications of electrolytic cells?