Hydrogen gas is not released when Zn is treated with dilute Nitric acid. Comment.

Explanation

### Step-by-Step Solution:

1. **Understanding the Reaction**: When zinc (Zn) is treated with dilute nitric acid (HNO₃), we expect a typical reaction where zinc displaces hydrogen ions (H⁺) from the acid, leading to the release of hydrogen gas (H₂).

2. **Expected Reaction**: The expected reaction can be represented as:
\[ \text{Zn} + 2\text{HNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + \text{H}_2 \]
However, this is not what occurs when zinc is treated with dilute nitric acid.

3. **Actual Reaction**: Instead of releasing hydrogen gas, the reaction proceeds as follows:
\[ \text{Zn} + 4\text{HNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + 2\text{H}_2\text{O} + 2\text{NO} \]
In this reaction, zinc nitrate (Zn(NO₃)₂) is formed along with water (H₂O) and nitrogen monoxide (NO) gas.

4. **Role of Nitric Acid**: The key reason hydrogen gas is not released is due to the strong oxidizing nature of nitric acid. Instead of allowing hydrogen to form, nitric acid oxidizes the hydrogen ions to water.

5. **Oxidation and Reduction**: In this reaction, nitric acid acts as an oxidizing agent, reducing itself in the process. Depending on the concentration of the nitric acid, it can be reduced to various nitrogen oxides (NO, NO₂, or N₂O).

6. **Conclusion**: Therefore, the absence of hydrogen gas when zinc reacts with dilute nitric acid is due to the strong oxidizing properties of nitric acid, which leads to the formation of water instead.