What You Need to Know

Key Concept Diagram

A galvanic (voltaic) cell converts chemical energy to electrical energy through spontaneous redox reactions

The anode is where oxidation occurs; the cathode is where reduction occurs (OIL RIG)

Electrolysis uses electrical energy to drive non-spontaneous chemical reactions

The standard electrode potential measures the tendency of a species to be reduced

Faraday's laws relate the amount of substance produced at an electrode to the charge passed

Key Vocabulary

Galvanic cell

An electrochemical cell that generates electrical energy from spontaneous chemical reactions

Electrolysis

Using electrical energy to drive a non-spontaneous chemical reaction

Electrode potential

The tendency of a species to gain electrons (be reduced) relative to a standard reference

Faraday constant

The charge of one mole of electrons: approximately 96,485 coulombs per mole

Knowledge Check

Select the correct answer for each question. Click "Check Answer" to see if you are right.

Question 1

In an electrochemical cell, the anode is the electrode where:

Reduction occurs Electrons enter the solution Oxidation occurs The electrolyte is stored

Question 2

Electrolysis requires:

A spontaneous chemical reaction Only gases as products No electrolyte An external electrical energy source to drive a non-spontaneous reaction

Question 3

Which application uses electrolysis on an industrial scale?

Electroplating metals to protect against corrosion Generating electricity in a battery Producing heat in a furnace Extracting oil from crude petroleum

Advanced Electrochemistry