In the equilibrium ` NH_(4) HS_(s) hArr NH_(3(g)) + H_(2) S_((g)) . `the forward reaction can be favoured by

Options

A. Adding some more `NH_(4) `HS
B. Adding some more `NH_(3)`
C. Removing some `NH_(3)` from the reaction mixture
D. Adding some more `H_(2)` S

Answer

To determine how to favor the forward reaction in the equilibrium:

\[ \text{NH}_4\text{HS}_{(s)} \rightleftharpoons \text{NH}_3_{(g)} + \text{H}_2\text{S}_{(g)} \]

we need to analyze the effects of changing concentrations of the reactants and products according to Le Chatelier's Principle.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction involves the solid ammonium hydrogen sulfide (NH₄HS) dissociating into gaseous ammonia (NH₃) and hydrogen sulfide (H₂S).

2. **Identify the Forward Reaction**:
The forward reaction is the dissociation of NH₄HS into NH₃ and H₂S. To favor this reaction, we need to either increase the concentration of reactants or decrease the concentration of products.

3. **Evaluating the Options**:
- **Option 1: Adding more NH₄HS**:
Adding more solid NH₄HS does not affect the equilibrium position since solids do not influence the equilibrium concentrations. Therefore, this option does not favor the forward reaction.

- **Option 2: Adding more NH₃**:
Adding more NH₃ increases the concentration of one of the products. According to Le Chatelier's Principle, this would shift the equilibrium to the left (towards the reactants), thus not favoring the forward reaction.

- **Option 3: Removing some NH₃ from the reaction mixture**:
Removing NH₃ decreases the concentration of one of the products. This would shift the equilibrium to the right (towards the products), thus favoring the forward reaction.

- **Option 4: Adding more H₂S**:
Similar to adding NH₃, adding more H₂S increases the concentration of a product, which would shift the equilibrium to the left, not favoring the forward reaction.

4. **Conclusion**:
The forward reaction can be favored by **removing some NH₃ from the reaction mixture**. This is the only option that effectively shifts the equilibrium to the right, promoting the formation of more products (NH₃ and H₂S).

### Final Answer:
The forward reaction can be favored by **removing some NH₃ from the reaction mixture**.