The exothermic formation of `ClF_3` is represented by the equations.
` Cl_2 (g) +3F_2 (g) hArr 2ClF_3 (g) : Delta ,H = -329 ` kJ
Which of the following will increase the quantity of `ClF_3` in an equilibrium mixture of `Cl_2 , F_2 and ClF_3` ?

Options

A. Adding ` F_2`
B. Increasing the volume of the container
C. Removing `Cl_2`
D. Increasing the temperature.

Explanation

To determine which action will increase the quantity of ClF3 in an equilibrium mixture of Cl2, F2, and ClF3, we can apply Le Chatelier's principle. Let's analyze the given reaction:

**Reaction:**
\[ Cl_2 (g) + 3F_2 (g) \rightleftharpoons 2ClF_3 (g) \]
**ΔH = -329 kJ (exothermic)**

### Step-by-Step Solution:

1. **Understanding the Reaction:**
The reaction shows that chlorine gas (Cl2) and fluorine gas (F2) react to form chlorine trifluoride (ClF3). Since the reaction is exothermic, it releases heat.

2. **Le Chatelier's Principle:**
According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.

3. **Evaluating Each Option:**
- **Option A: Adding F2**
- When F2 is added, the concentration of F2 increases. This causes the reaction to shift to the right to consume the added F2, thereby producing more ClF3.
- **Effect:** Increases ClF3.

- **Option B: Increasing the volume of the container**
- Increasing the volume decreases the concentration of all gases. According to the reaction, there are 4 moles of reactants (1 Cl2 + 3 F2) and 2 moles of products (2 ClF3). The reaction will shift to the left (towards the side with more moles) to counteract the decrease in concentration.
- **Effect:** Decreases ClF3.

- **Option C: Removing Cl2**
- Removing Cl2 decreases its concentration. The system will respond by shifting to the left to produce more Cl2, which results in a decrease in ClF3.
- **Effect:** Decreases ClF3.

- **Option D: Increasing the temperature**
- Since the reaction is exothermic, increasing the temperature will shift the equilibrium to the left (towards the reactants) to absorb the added heat.
- **Effect:** Decreases ClF3.

4. **Conclusion:**
The only action that increases the quantity of ClF3 in the equilibrium mixture is **Option A: Adding F2**.

### Final Answer:
**Adding F2 will increase the quantity of ClF3 in the equilibrium mixture.**

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