Magnesium is produced commercially by electrolysis from a molten salt using a cell similar to the one shown here. (a) What salt is used as the electrolyte? (b) Which electrode is the anode, and which one is the cathode? (c) Write the overall cell reaction and individual half-reactions. (d) What precautions would need to be taken with respect to the magnesium formed? [Section 20.9]
One Class Solution:- a) Magnesium chloride must be heated until it is molten before it will conduct electricity. Electrolysis separates the molten ionic compound into its elements.
b, c)Mg2+ + 2e-→Mg (magnesium metal at the (-) cathode). Steel electrodes.
2Cl- - 2e- →Cl2 (chlorine gas at the (+) anode)- Carbon electrode.
Mg is an active metal- >It must be separated from the Cl2(g) that is also formed by electrolysis or MgCl2 will spontaneously reformed.
Magnesium is produced commercially by electrolysis from a molten salt using a cell similar to the one shown here. (a) What salt is used as the electrolyte? (b) Which electrode is the anode, and which one is the cathode? (c) Write the overall cell reaction and individual half-reactions. (d) What precautions would need to be taken with respect to the magnesium formed? [Section 20.9]
One Class Solution:- a) Magnesium chloride must be heated until it is molten before it will conduct electricity. Electrolysis separates the molten ionic compound into its elements.
b, c)Mg2+ + 2e-→Mg (magnesium metal at the (-) cathode). Steel electrodes.
2Cl- - 2e- →Cl2 (chlorine gas at the (+) anode)- Carbon electrode.
Mg is an active metal- >It must be separated from the Cl2(g) that is also formed by electrolysis or MgCl2 will spontaneously reformed.
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