As per Lechatelier's Principle any stress applied on the equilibrium state is minimised by shifting of equilibrium.
Increase in volume of container shifts the equilibrium in forward direction in the case of ____

Options

A. `N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))`
B. `CaCO_(3(s)) hArr CaO_((s)) + CO_(2(g))`
C. `N_(2(g)) + O_(2(g)) hArr 2NO_((g))`
D. `C_(2) H_(5) OH_((l)) + CH_(3)"COOH"_((l)) hArr CH_(3) "COOC"_(2) H_(5(l)) + H_(2)O_((l))`

Answer

To solve the question regarding Le Chatelier's Principle and the effect of increasing the volume of a container on equilibrium, we can follow these steps:

### Step-by-Step Solution:

1. **Understand Le Chatelier's Principle**: This principle states that if an external stress is applied to a system at equilibrium, the system will adjust itself to counteract that stress and restore a new equilibrium.

2. **Identify the Effect of Volume Change**: Increasing the volume of a container decreases the pressure of the system. According to Le Chatelier's Principle, the equilibrium will shift in the direction that increases the pressure.

3. **Analyze the Reactions Given**: We need to look at the provided reactions and determine which one has a greater number of gaseous moles on the product side compared to the reactant side. This will help us identify which reaction will shift forward when the volume is increased.

- **Reaction 1**: N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
- Reactants: 1 + 3 = 4 moles
- Products: 2 moles
- **Net Effect**: Decrease in moles, will not favor forward direction.

- **Reaction 2**: CaCO₃(s) ⇌ CaO(s) + CO₂(g)
- Reactants: 0 moles (solid)
- Products: 1 mole (gaseous)
- **Net Effect**: Increase in moles, will favor forward direction.

- **Reaction 3**: N₂(g) + O₂(g) ⇌ 2NO(g)
- Reactants: 1 + 1 = 2 moles
- Products: 2 moles
- **Net Effect**: No change in moles, will not favor forward direction.

- **Reaction 4**: C₂H₅OH(l) + CH₃COOH(l) ⇌ C₄H₈O₂(l) + H₂O(l)
- All components are liquids, so pressure change does not apply.

4. **Conclusion**: The only reaction that will shift in the forward direction upon increasing the volume of the container is the second one (CaCO₃(s) ⇌ CaO(s) + CO₂(g)), as it results in an increase in the number of gaseous moles.

### Final Answer:
The equilibrium will shift in the forward direction in the case of the decomposition of calcium carbonate (CaCO₃(s) ⇌ CaO(s) + CO₂(g)) when the volume of the container is increased.

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