`Zn+H_(2)SO_(4)rarrZnSO_(4)+H_(2)`
Zn undergoes -

Options

A. Reduction
B. Oxidation
C. Both oxidation and reduction
D. None of these

Answer

To determine whether zinc (Zn) undergoes oxidation or reduction in the reaction with sulfuric acid (H₂SO₄), we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction given is:
\[ \text{Zn} + \text{H}_2\text{SO}_4 \rightarrow \text{ZnSO}_4 + \text{H}_2 \]

### Step 2: Identify the oxidation states of the elements
- In elemental form, the oxidation state of zinc (Zn) is **0**.
- In zinc sulfate (ZnSO₄), we need to determine the oxidation state of zinc. The sulfate ion (SO₄²⁻) has a charge of **-2**. Since the compound is neutral, the oxidation state of zinc (let's denote it as X) can be calculated as follows:
\[ X + (-2) = 0 \implies X = +2 \]
Thus, the oxidation state of zinc in ZnSO₄ is **+2**.

### Step 3: Determine the change in oxidation state
- Zinc changes from an oxidation state of **0** (in Zn) to **+2** (in ZnSO₄).
- This indicates that zinc has lost electrons.

### Step 4: Conclusion about the reaction
Since the oxidation state of zinc increases from 0 to +2, this process is classified as **oxidation**. In oxidation, there is a loss of electrons.

### Final Answer
Zinc (Zn) undergoes **oxidation** in the reaction with sulfuric acid.

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