For the reaction `H_(2)(g)+I_(2)(g) hArr 2HI(g)`, the equilibrium can be shifted in favour of product by

Options

A. Increasing the `[H_(2)]`
B. Increasing the pressure
C. Increasing the `[I_(2)]`
D. By using the catalyst

Explanation

To determine how the equilibrium of the reaction \( H_2(g) + I_2(g) \rightleftharpoons 2HI(g) \) can be shifted in favor of the products, we can apply Le Chatelier's principle. Here’s a step-by-step solution:

### Step 1: Understand the Reaction
The reaction involves hydrogen gas (\( H_2 \)) and iodine gas (\( I_2 \)) reacting to form hydrogen iodide (\( HI \)).

### Step 2: Identify the Equilibrium Expression
The equilibrium expression for this reaction can be written as:
\[ K_c = \frac{[HI]^2}{[H_2][I_2]} \]
Where \( K_c \) is the equilibrium constant.

### Step 3: Apply Le Chatelier's Principle
Le Chatelier's principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.

### Step 4: Analyze the Options
1. **Increasing the concentration of \( H_2 \)**:
- If we increase the concentration of a reactant, the equilibrium will shift to the right (towards the products) to consume the added \( H_2 \).
- **Effect**: Shift to products.

2. **Increasing the concentration of \( I_2 \)**:
- Similar to increasing \( H_2 \), increasing \( I_2 \) will also shift the equilibrium to the right to produce more \( HI \).
- **Effect**: Shift to products.

3. **Increasing the pressure**:
- The reaction has 2 moles of gas on both sides (2 moles of \( H_2 \) and \( I_2 \) on the left and 2 moles of \( HI \) on the right). Therefore, increasing the pressure will not favor either side since the number of moles is the same.
- **Effect**: No shift.

4. **Using a catalyst**:
- A catalyst speeds up the rate of both the forward and reverse reactions equally but does not affect the position of equilibrium.
- **Effect**: No shift.

### Step 5: Conclusion
The equilibrium can be shifted in favor of the products by:
- Increasing the concentration of \( H_2 \)
- Increasing the concentration of \( I_2 \)

Thus, the correct answers are:
- Increasing the concentration of \( H_2 \)
- Increasing the concentration of \( I_2 \)