`Zn(s)+2HCl to ZnCl_(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 determine the type of reaction represented by the equation \( \text{Zn(s)} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \), we can analyze the components and changes occurring in the reaction step by step.

### Step 1: Identify the Reactants and Products
- The reactants are zinc (Zn) in solid form and hydrochloric acid (HCl).
- The products are zinc chloride (ZnCl2) and hydrogen gas (H2).

**Hint:** Look at the substances involved in the reaction to understand what is being transformed.

### Step 2: Determine the Reactivity of the Elements
- Zinc (Zn) is a metal and is more reactive than hydrogen (H) in this context. This means that zinc can displace hydrogen from hydrochloric acid.

**Hint:** Recall the reactivity series of metals to assess which element can displace another.

### Step 3: Classify the Reaction Type
- Since zinc displaces hydrogen from hydrochloric acid, this is classified as a **displacement reaction** (also known as a single replacement reaction).

**Hint:** Think about whether one element is replacing another in the reaction.

### Step 4: Analyze Oxidation States
- In the reactants:
- Zinc (Zn) is in the elemental state with an oxidation state of 0.
- Hydrogen in HCl has an oxidation state of +1.
- Chlorine in HCl has an oxidation state of -1.

- In the products:
- In ZnCl2, zinc has an oxidation state of +2 (since Cl is -1).
- Hydrogen in H2 has an oxidation state of 0.

**Hint:** Check the oxidation states of the elements before and after the reaction to see if any changes occur.

### Step 5: Identify Oxidation and Reduction
- Zinc's oxidation state increases from 0 to +2, indicating that zinc is **oxidized**.
- Hydrogen's oxidation state decreases from +1 to 0, indicating that hydrogen is **reduced**.

**Hint:** Remember that oxidation involves an increase in oxidation state, while reduction involves a decrease.

### Step 6: Conclude the Type of Reaction
- Since both oxidation and reduction occur simultaneously, this reaction is classified as a **redox reaction** (reduction-oxidation reaction).

**Hint:** Look for changes in oxidation states to identify redox reactions.

### Final Answer
The reaction \( \text{Zn(s)} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \) is a **displacement reaction** and also a **redox reaction**.