The hydrolysis of `NCl_3` by `H_2 O` produces

Options

A. `NH_2NH_2 and HOCl`
B. `NH_2OH and HOCl`
C. `NH_2Cl and HOCl`
D. `NH_4OH and HOCl`

Answer

To solve the question regarding the hydrolysis of \( NCl_3 \) by \( H_2O \), we can follow these steps:

### Step 1: Write the chemical equation for hydrolysis
The hydrolysis of nitrogen trichloride (\( NCl_3 \)) in the presence of water (\( H_2O \)) can be represented by the following equation:

\[ NCl_3 + H_2O \rightarrow NH_4OH + HOCl \]

### Step 2: Balance the equation
Now, we need to ensure that the equation is balanced. In this case, we can see that:

- On the left side, we have 1 nitrogen atom, 3 chlorine atoms, and 2 hydrogen atoms from water.
- On the right side, we have 1 nitrogen atom in \( NH_4OH \) and 1 in \( HOCl \), totaling 2 nitrogen atoms.

To balance the equation, we can adjust the coefficients:

\[ NCl_3 + 3 H_2O \rightarrow NH_4OH + 3 HOCl \]

### Step 3: Identify the products
From the balanced equation, we can identify the products of the hydrolysis reaction:

- \( NH_4OH \) (ammonium hydroxide)
- \( HOCl \) (hypochlorous acid)

### Conclusion
Thus, the hydrolysis of \( NCl_3 \) by \( H_2O \) produces \( NH_4OH \) and \( HOCl \).

### Final Answer
The correct products of the hydrolysis of \( NCl_3 \) by \( H_2O \) are \( NH_4OH \) and \( HOCl \).