`10ml` of compound containing 'N' and 'O' is mixed with `30ml` of `H_(2)` to produce `H_(2)O (l)` and `10ml` of `N_(2)(g)`. Molecular formula of compound if both reactants completely, is

Options

A. `N_(2)O`
B. `NO_(2)`
C. `N_(2)O_(3)`
D. `N_(2)O_(5)`

Explanation

To determine the molecular formula of the compound containing nitrogen (N) and oxygen (O) that reacts with hydrogen (H₂) to produce water (H₂O) and nitrogen gas (N₂), we can follow these steps:

### Step 1: Analyze the Reaction
We know that:
- 10 ml of the compound reacts with 30 ml of H₂.
- The products are 10 ml of N₂ and H₂O.

### Step 2: Use the Volume Ratio
At standard temperature and pressure (STP), the volume of gases can be directly related to the number of moles.
- The volume ratio of the gases suggests that:
- 1 volume of the compound reacts with 3 volumes of H₂ to produce 1 volume of N₂ and some volume of H₂O.

### Step 3: Write the Balanced Chemical Equation
From the information given, we can write the unbalanced equation:
\[ \text{Compound} + 3H_2 \rightarrow N_2 + H_2O \]

### Step 4: Identify the Compound
Let’s denote the compound as \( \text{N}_x\text{O}_y \).
From the reaction, we can deduce:
- For every 1 mole of the compound, 3 moles of H₂ are required.
- The products indicate that the nitrogen in the compound is converted to N₂.

### Step 5: Determine the Molecular Formula
Assuming the compound is \( \text{N}_2\text{O}_3 \):
- The balanced equation would be:
\[ \text{N}_2\text{O}_3 + 3H_2 \rightarrow 3H_2O + N_2 \]
- This means that 1 mole of \( \text{N}_2\text{O}_3 \) reacts with 3 moles of H₂ to produce 3 moles of H₂O and 1 mole of N₂.

### Conclusion
The molecular formula of the compound is \( \text{N}_2\text{O}_3 \).

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