In the preparation of `HNO_(3)`, we get NO gas by catalytic oxidation of ammonia . The moles of No produced by the oxidation of two moles of `NH_(3)` will be ……… .

Options

A. 2
B. 3
C. 4
D. 6

Explanation

To solve the problem of determining the moles of NO produced by the catalytic oxidation of two moles of NH₃, we can follow these steps:

### Step-by-Step Solution:

1. **Write the Balanced Chemical Equation**:
The balanced equation for the catalytic oxidation of ammonia (NH₃) is:
\[ 4 \, \text{NH}_3 + 5 \, \text{O}_2 \rightarrow 4 \, \text{NO} + 6 \, \text{H}_2\text{O} \]

2. **Identify the Stoichiometric Ratios**:
From the balanced equation, we can see that 4 moles of NH₃ produce 4 moles of NO. This gives us a stoichiometric ratio of:
\[ \frac{4 \, \text{NO}}{4 \, \text{NH}_3} = 1 \]
This means that for every mole of NH₃, one mole of NO is produced.

3. **Calculate the Moles of NO from Given Moles of NH₃**:
If we have 2 moles of NH₃, we can use the stoichiometric ratio to find the moles of NO produced:
\[ \text{Moles of NO} = 2 \, \text{moles of NH}_3 \times \frac{4 \, \text{NO}}{4 \, \text{NH}_3} = 2 \, \text{moles of NO} \]

4. **Final Answer**:
Therefore, the moles of NO produced by the oxidation of 2 moles of NH₃ is:
\[ \text{Answer} = 2 \, \text{moles of NO} \]

### Summary:
The moles of NO produced by the oxidation of 2 moles of NH₃ is **2 moles**.