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 determine the moles of NO produced from the oxidation of 2 moles of NH3, we first need to write the balanced chemical equation for the reaction.

### Step 1: Write the balanced chemical equation
The catalytic oxidation of ammonia (NH3) can be represented by the following balanced equation:

\[ 4 \, \text{NH}_3(g) + 5 \, \text{O}_2(g) \xrightarrow{\text{catalyst}} 4 \, \text{NO}(g) + 6 \, \text{H}_2O(l) \]

### Step 2: Identify the stoichiometric coefficients
From the balanced equation, we can see that 4 moles of NH3 produce 4 moles of NO. This means that the ratio of NH3 to NO is 1:1.

### Step 3: Calculate the moles of NO produced from 2 moles of NH3
Since the ratio of NH3 to NO is 1:1, if we start with 2 moles of NH3, we will produce an equal amount of NO:

\[ \text{Moles of NO produced} = \text{Moles of NH}_3 \times \left(\frac{4 \, \text{moles NO}}{4 \, \text{moles NH}_3}\right) = 2 \, \text{moles NH}_3 \times 1 = 2 \, \text{moles NO} \]

### Final Answer
Thus, the moles of NO produced by the oxidation of 2 moles of NH3 will be **2 moles**.

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