`N_(2)(g) +3H_(2)(g) hArr 2NH_(3)(g),`
In the reaction given above, the addition of small amount of an inert gas at constant pressure will shift the equilibrium towardss which side of

Options

A. LHS(Left hand side)
B. RHS(Right hand side)
C. Neither side
D. Either side

Explanation

To solve the problem regarding the equilibrium shift in the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \) upon the addition of an inert gas at constant pressure, we can follow these steps:

### Step 1: Understand the Reaction
The given reaction involves nitrogen and hydrogen gases reacting to form ammonia. The balanced equation shows:
- Reactants: 1 mole of \( N_2 \) and 3 moles of \( H_2 \) (total 4 moles)
- Products: 2 moles of \( NH_3 \)

### Step 2: Identify the Effect of Inert Gas Addition
According to Le Chatelier's principle, if a system at equilibrium experiences a change (like the addition of an inert gas), the system will adjust to counteract that change and restore equilibrium.

### Step 3: Analyze the Change in Moles
When an inert gas is added at constant pressure:
- The total pressure of the system increases, but the partial pressures of the reactants and products remain unchanged.
- Since the addition of an inert gas does not participate in the reaction, it does not change the concentrations of the reactants or products.

### Step 4: Determine the Direction of Equilibrium Shift
At constant pressure, the equilibrium will shift towards the side with more moles of gas. In this reaction:
- Reactants: 4 moles (1 mole of \( N_2 \) + 3 moles of \( H_2 \))
- Products: 2 moles (2 moles of \( NH_3 \))

Since there are more moles of gas on the reactant side (4 moles) compared to the product side (2 moles), the equilibrium will shift towards the left side (the reactants).

### Conclusion
The addition of a small amount of inert gas at constant pressure will shift the equilibrium towards the left side (the reactants).

### Final Answer
The equilibrium will shift towards the left-hand side.

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