The exothermic formation of `ClF_(3)` is represented by thr equation:
`Cl_(2)(g)+3F_(2)(g) hArr 2ClF_(3)(g), DeltaH=-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. Increasing the temperature
B. Removing `Cl_(2)`
C. Increasing the volume of the container
D. Adding `F_(2)`

Explanation

To solve the problem, we need to analyze the given equilibrium reaction and how changes in conditions affect the quantity of the product, ClF₃.

### Step-by-Step Solution:

1. **Identify the Reaction**: The reaction given is:
\[ \text{Cl}_2(g) + 3\text{F}_2(g) \rightleftharpoons 2\text{ClF}_3(g) \]
This is an exothermic reaction with a change in enthalpy (\(\Delta H\)) of -329 kJ.

2. **Understand 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 equilibrium will shift to counteract that change.

3. **Analyze the Changes**: We want to increase the quantity of ClF₃ in the equilibrium mixture. To do this, we can:
- Increase the concentration of reactants (Cl₂ or F₂).
- Decrease the concentration of products (ClF₃).
- Change the temperature or pressure, but in this case, we focus on concentration changes.

4. **Consider the Options**: The question asks which of the following will increase the quantity of ClF₃. The most effective way to shift the equilibrium to the right (towards the products) is to increase the concentration of the reactants.

5. **Adding F₂**: If we add more F₂ to the system, the equilibrium will shift to the right to consume the added F₂, resulting in the formation of more ClF₃. This is because more F₂ will react with Cl₂ to produce ClF₃.

6. **Conclusion**: Therefore, the action that will increase the quantity of ClF₃ in the equilibrium mixture is the addition of F₂.

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

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