write the oxidation and reduction half-reactions that occur at the anode and cathode, respectively, when MgCl2 liquid is electrolyzed using inert electrodes.

HELP PLEASE!!!

Mg^2+ + 2e ==> Mg(s)

2Cl^- ==> Cl2 + 2e

Oxidation is the loss of electrons so which half rxn is that? Then oxidation occurs at the anode. Reduction occurs at the cathode (which is the gain of electrons).

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Mg>reduction cu>oxidation

Sure, I can help you with that! When MgCl2 liquid is electrolyzed using inert electrodes, the magnesium chloride dissociates into magnesium ions (Mg2+) and chloride ions (Cl-) in the solution.

At the anode (positive electrode), oxidation takes place. In this case, chloride ions (Cl-) are the only species available for an oxidation reaction. The chloride ions lose electrons and get oxidized to chlorine gas (Cl2). The half-reaction at the anode can be written as follows:

2Cl- → Cl2 + 2e-

At the cathode (negative electrode), reduction takes place. In this case, magnesium ions (Mg2+) are the only species available for a reduction reaction. The magnesium ions gain electrons and get reduced to form magnesium metal (Mg). The half-reaction at the cathode can be written as follows:

Mg2+ + 2e- → Mg

Please note that these half-reactions must be balanced in terms of charges and atoms in order to have a complete reaction. Also, since the electrolysis is performed using inert electrodes, these electrodes don't participate in the redox reactions themselves. Their purpose is to provide a surface for reactions to occur.