Questions: Study this chemical reaction: CuCl2(aq) + Mg(s) -> MgCl2(aq) + Cu(s) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Study this chemical reaction:
CuCl2(aq) + Mg(s) -> MgCl2(aq) + Cu(s)

Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Transcript text: Study this chemical reaction: \[ \mathrm{CuCl}_{2}(\mathrm{aq})+\mathrm{Mg}(s) \rightarrow \mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{Cu}(s) \] Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Solution

Solution Steps

Step 1: Identify the Elements Involved in the Reaction

The given chemical reaction is: \[ \mathrm{CuCl}_{2}(\mathrm{aq})+\mathrm{Mg}(s) \rightarrow \mathrm{MgCl}_{2}(\mathrm{aq})+\mathrm{Cu}(s) \] In this reaction, copper (Cu) and magnesium (Mg) are the elements undergoing oxidation and reduction.

Step 2: Determine the Oxidation and Reduction Processes

Oxidation is the loss of electrons. In this reaction, magnesium (Mg) is oxidized as it loses electrons to form magnesium ions (\(\mathrm{Mg}^{2+}\)).
Reduction is the gain of electrons. Copper ions (\(\mathrm{Cu}^{2+}\)) are reduced as they gain electrons to form copper metal (Cu).

Step 3: Write the Oxidation Half-Reaction

The oxidation half-reaction involves magnesium losing two electrons: \[ \mathrm{Mg}(s) \rightarrow \mathrm{Mg}^{2+}(aq) + 2e^{-} \]

Step 4: Write the Reduction Half-Reaction

The reduction half-reaction involves copper ions gaining two electrons: \[ \mathrm{Cu}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Cu}(s) \]

Final Answer

Oxidation half-reaction: \(\boxed{\mathrm{Mg}(s) \rightarrow \mathrm{Mg}^{2+}(aq) + 2e^{-}}\)
Reduction half-reaction: \(\boxed{\mathrm{Cu}^{2+}(aq) + 2e^{-} \rightarrow \mathrm{Cu}(s)}\)

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