`Zn+conc.HNO_(3) rarr Zn(NO_(3))_(2)+X+H_(2)O`
`Zn+dil.HNO_(3) rarr Zn(NO_(3))_(2)+Y+H_(2)O`
Compounds X and Y are respectively:

Options

A. `N_(2)O, NO`
B. `NO_(2), N_(2)O`
C. `N_(2)O,NO_(2)`
D. `NO_(2),NO`

Explanation

To solve the question, we need to analyze the reactions of zinc (Zn) with concentrated and dilute nitric acid (HNO3) and identify the products formed in each case.

### Step 1: Reaction of Zinc with Concentrated HNO3

When zinc reacts with concentrated nitric acid, it acts as a strong oxidizing agent. The reaction can be represented as:

\[ \text{Zn} + \text{conc. HNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + \text{X} + \text{H}_2\text{O} \]

In this reaction, zinc is oxidized, and the nitrogen in nitric acid is reduced to nitrogen dioxide (NO2). The balanced equation for this reaction is:

\[ \text{4 Zn} + \text{10 HNO}_3 \rightarrow \text{4 Zn(NO}_3\text{)}_2 + \text{2 NO}_2 + \text{5 H}_2\text{O} \]

Thus, the product X formed in this reaction is nitrogen dioxide (NO2).

### Step 2: Reaction of Zinc with Dilute HNO3

Now, when zinc reacts with dilute nitric acid, the reaction is milder, and the nitrogen in nitric acid is reduced to a lower oxidation state. The reaction can be represented as:

\[ \text{Zn} + \text{dil. HNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + \text{Y} + \text{H}_2\text{O} \]

In this case, the nitrogen is reduced to nitrous oxide (N2O). The balanced equation for this reaction is:

\[ \text{Zn} + \text{4 HNO}_3 \rightarrow \text{Zn(NO}_3\text{)}_2 + \text{2 N}_2\text{O} + \text{2 H}_2\text{O} \]

Thus, the product Y formed in this reaction is nitrous oxide (N2O).

### Conclusion

From the above analysis, we can conclude that:

- Compound X (from the reaction with concentrated HNO3) is NO2.
- Compound Y (from the reaction with dilute HNO3) is N2O.

Therefore, the answer is:
- X = NO2
- Y = N2O