`Fe(l)hArrFe(s)`
Above equilibrium is favoured at :

Options

A. high pressure, low temperature
B. high pressure, high temperature
C. low pressure, high temperature
D. low pressure, low temperature

Answer

To determine the conditions under which the equilibrium `Fe(l) ⇌ Fe(s)` is favored, we need to analyze the nature of the reaction and apply Le Chatelier's principle.

### Step-by-Step Solution:

1. **Identify the Reaction Type**:
The reaction involves the conversion of liquid iron (Fe(l)) to solid iron (Fe(s)). This process is a phase change from liquid to solid.

2. **Determine the Heat Exchange**:
The conversion from liquid to solid (freezing) releases heat. Therefore, this reaction is exothermic. In exothermic reactions, the enthalpy change (ΔH) is negative.

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

4. **Effect of Temperature**:
- For exothermic reactions, increasing the temperature shifts the equilibrium to favor the endothermic direction (the reverse reaction, which is melting in this case).
- Conversely, decreasing the temperature will favor the forward reaction (solid formation). Therefore, lower temperatures will favor the formation of solid iron.

5. **Effect of Pressure**:
- In this reaction, the volume decreases when liquid iron converts to solid iron (since solids occupy less volume than liquids).
- According to the principle, increasing pressure favors the side of the reaction that has fewer moles of gas or, in this case, the side with less volume. Therefore, high pressure will also favor the formation of solid iron.

6. **Conclusion**:
To favor the equilibrium towards solid iron, we need to have low temperature and high pressure conditions.

### Final Answer:
The equilibrium `Fe(l) ⇌ Fe(s)` is favored at **high pressure and low temperature**.

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