`Cl_(2)` on reaction with excess of `NH_(3)` gives

Options

A. `NH_(4) Cl + N_(2)`
B. `NCl_3 + HCl`
C. `NH_4 Cl` only
D. `NH_4 Cl + NCl_(3)`

Answer

To solve the problem of what products are formed when chlorine gas (Cl₂) reacts with excess ammonia (NH₃), we can follow these steps:

### Step 1: Write the Reactants
The reactants in this reaction are chlorine gas (Cl₂) and ammonia (NH₃).

### Step 2: Identify the Reaction
When chlorine reacts with ammonia, it can lead to the formation of ammonium chloride (NH₄Cl) and nitrogen gas (N₂). This reaction typically occurs when chlorine is in excess, which influences the products formed.

### Step 3: Write the Balanced Chemical Equation
The balanced chemical equation for the reaction can be written as follows:
\[ 3 Cl_2 + 8 NH_3 \rightarrow 6 NH_4Cl + N_2 \]
This indicates that three moles of chlorine gas react with eight moles of ammonia to produce six moles of ammonium chloride and one mole of nitrogen gas.

### Step 4: Determine the Products
From the balanced equation, we can see that the products formed are:
- Ammonium chloride (NH₄Cl)
- Nitrogen gas (N₂)

### Step 5: Conclusion
Thus, when Cl₂ reacts with excess NH₃, the products formed are ammonium chloride and nitrogen gas. Therefore, the correct answer to the question is:
**NH₄Cl + N₂**