Ch.18 - ElectrochemistryWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Magnesium, the element, is produced commercially by electrolysis from a molten salt (the "electrolyte") using a cell similar to the one shown below.Recall that in an electrolytic cell the anode is giv

Solution: Magnesium, the element, is produced commercially by electrolysis from a molten salt (the "electrolyte") using a cell similar to the one shown below.Recall that in an electrolytic cell the anode is giv

Problem

Magnesium, the element, is produced commercially by electrolysis from a molten salt (the "electrolyte") using a cell similar to the one shown below.

A diagram shows a box containing electrolyte with two electrodes in it, one steel and one carbon.  The negative end of a voltage source is attached to the steel electrode while the positive end is attached to the carbon electrode.  There is a thin layer of liquid Mg near the steel electrode.  Bubbles from around the carbon electrode are Cl2 (gas), which escapes through an outflow tube.

Recall that in an electrolytic cell the anode is given the + sign and the cathode is given the - sign, which is the opposite of what we see in batteries. What half-reaction occurs at the anode in this electrolytic cell?

Solution

We are asked for the half-reaction that occurs at the anode in this electrolytic cell.


We’re given the following electrochemical cell:

A diagram shows a box containing electrolyte with two electrodes in it, one steel and one carbon.  The negative end of a voltage source is attached to the steel electrode while the positive end is attached to the carbon electrode.  There is a thin layer of liquid Mg near the steel electrode.  Bubbles from around the carbon electrode are Cl2 (gas), which escapes through an outflow tube.


Since a voltage source is given, this is an electrolytic cellwhere a nonspontaneous process is occurring. 

Since the process is nonspontaneous, an outside energy source provides energy for it to occur.


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