When `P_(4)` reacts with `HNO_(3)` products formed is/are:

Options

A. `H_(3)PO_(4)`
B. `NO`
C. `N_(2)O_(5)`
D. `NO_(2)`

Answer

To determine the products formed when \( P_4 \) reacts with \( HNO_3 \), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are tetraphosphorus (\( P_4 \)) and nitric acid (\( HNO_3 \)).

### Step 2: Write the Reaction
When \( P_4 \) reacts with concentrated \( HNO_3 \), the general reaction can be represented as:
\[ P_4 + HNO_3 \rightarrow H_3PO_4 + NO_2 + H_2O \]
This indicates that phosphoric acid (\( H_3PO_4 \)), nitrogen dioxide (\( NO_2 \)), and water (\( H_2O \)) are produced.

### Step 3: Balance the Reaction
To balance the reaction, we need to ensure that the number of atoms for each element is the same on both sides. The balanced equation is:
\[ P_4 + 10 HNO_3 \rightarrow 4 H_3PO_4 + 10 NO_2 + 2 H_2O \]
This shows that for every molecule of \( P_4 \), we need 10 molecules of \( HNO_3 \) to produce 4 molecules of \( H_3PO_4 \), 10 molecules of \( NO_2 \), and 2 molecules of \( H_2O \).

### Step 4: Identify the Products
From the balanced equation, we can identify the products formed:
1. Phosphoric Acid (\( H_3PO_4 \))
2. Nitrogen Dioxide (\( NO_2 \))

### Conclusion
The products formed when \( P_4 \) reacts with \( HNO_3 \) are \( H_3PO_4 \) and \( NO_2 \).

### Final Answer
The correct options for the products formed are:
- \( H_3PO_4 \) (Phosphoric Acid)
- \( NO_2 \) (Nitrogen Dioxide)

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