`Mg(s)+2HCl to MgCl_(2)+H_(2)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To analyze the reaction \( \text{Mg}(s) + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2 \) and determine the type of reaction, we can follow these steps:

### Step 1: Identify the Reactants and Products
The reactants in this reaction are magnesium (Mg) in solid form and hydrochloric acid (HCl). The products are magnesium chloride (MgCl2) and hydrogen gas (H2).

### Step 2: Determine the Oxidation States
- For magnesium (Mg) in its elemental form, the oxidation state is 0.
- In hydrochloric acid (HCl), the oxidation state of hydrogen (H) is +1.
- In magnesium chloride (MgCl2), the oxidation state of magnesium (Mg) is +2.
- In hydrogen gas (H2), the oxidation state of hydrogen (H) is 0.

### Step 3: Analyze Changes in Oxidation States
- Magnesium (Mg) changes from an oxidation state of 0 to +2, indicating that it is oxidized.
- Hydrogen (H) changes from +1 in HCl to 0 in H2, indicating that it is reduced.

### Step 4: Identify the Type of Reaction
Since we have both oxidation (Mg) and reduction (H) occurring simultaneously, this is classified as a redox reaction. Specifically, it is an intermolecular redox reaction because the oxidation and reduction processes are occurring between different molecules.

### Step 5: Eliminate Other Options
- **Displacement Reaction**: This reaction can also be considered a single displacement reaction where magnesium displaces hydrogen from hydrochloric acid.
- **Thermal Combination/Decomposition**: These options are eliminated since there is no indication of thermal energy being involved.

### Conclusion
The type of reaction is an **intermolecular redox reaction**.