Equal moles of `F_(2(g)) and Cl_(2(g))` are introduced into a sealed container and heated to temperature T to attain the following equilibria. `Cl_(2(g)) + F_(2(g)) hArr 2ClF_((g)) `.` in which direction the equilibrium will shift if concentration of F2 increased?

Answer

To solve the question regarding the equilibrium shift when the concentration of \( F_2 \) is increased, we can follow these steps:

### Step 1: Write the Equilibrium Reaction
The equilibrium reaction given is:
\[ Cl_2(g) + F_2(g) \rightleftharpoons 2ClF(g) \]

### Step 2: Identify the Change in Concentration
The question states that the concentration of \( F_2 \) is increased. This means that the amount of one of the reactants is being raised.

### Step 3: Apply Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the equilibrium will shift in a direction that counteracts the change.

In this case, since we are increasing the concentration of \( F_2 \):
- The system will respond by shifting the equilibrium to the right (towards the products) to consume some of the added \( F_2 \).

### Step 4: Conclusion
Therefore, when the concentration of \( F_2 \) is increased, the equilibrium will shift to the right, favoring the formation of \( ClF \).

### Final Answer
The equilibrium will shift to the right (towards the formation of \( ClF \)) when the concentration of \( F_2 \) is increased.

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