The electrolysis of molten KCl. `MgCl_(2) . 6H_(2)O` gives

Options

A. Mg only
B. K only
C. K and Mg only
D. Mg, K and `Cl_(2)`

Answer

To solve the question regarding the electrolysis of molten KCl and MgCl₂·6H₂O, we will follow these steps:

### Step 1: Understand Electrolysis
Electrolysis is a chemical process that uses electric current to drive a non-spontaneous reaction. In this case, we are dealing with the electrolysis of ionic compounds, which will break down into their constituent ions when molten or dissolved in water.

### Step 2: Identify the Components
The given compound is MgCl₂·6H₂O. When we perform electrolysis, we need to consider the ions produced from this compound:
- MgCl₂ dissociates into Mg²⁺ and Cl⁻ ions.
- The presence of water (H₂O) can also lead to the production of H⁺ and OH⁻ ions, but since we are focusing on the molten state, we will primarily consider the ions from MgCl₂.

### Step 3: Write the Ionization Equation
When MgCl₂ is melted, it ionizes as follows:
\[ \text{MgCl}_2 \rightarrow \text{Mg}^{2+} + 2\text{Cl}^- \]

### Step 4: Electrolysis Process
During electrolysis:
- At the cathode (negative electrode), reduction occurs. The Mg²⁺ ions will gain electrons to form magnesium metal (Mg).
- At the anode (positive electrode), oxidation occurs. The Cl⁻ ions will lose electrons to form chlorine gas (Cl₂).

### Step 5: Products of Electrolysis
From the above reactions, we can summarize the products:
- Magnesium metal (Mg) is produced at the cathode.
- Chlorine gas (Cl₂) is produced at the anode.

### Step 6: Conclusion
Thus, the electrolysis of molten MgCl₂·6H₂O gives magnesium (Mg) and chlorine gas (Cl₂). Therefore, the correct answer is option 4: Mg, K, and Cl₂.

### Final Answer
The electrolysis of molten KCl and MgCl₂·6H₂O gives magnesium (Mg), potassium (K), and chlorine gas (Cl₂).

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