If Ar is added to the equilibrium `N_2(g) +3H_2(g) hArr 2NH_3` at constant volume , the equilibrium will

Options

A. Shift in forward direction
B. Shift in reverse direction
C. Not shift in any direction
D. All are incorrect

Answer

To solve the question regarding the effect of adding argon (an inert gas) to the equilibrium reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \) at constant volume, we can follow these steps:

### Step 1: Understand the Equilibrium System
The equilibrium reaction involves nitrogen gas (\( N_2 \)), hydrogen gas (\( H_2 \)), and ammonia gas (\( NH_3 \)). The equilibrium can be affected by changes in concentration, pressure, and temperature.

**Hint:** Identify the components of the equilibrium system and their states.

### Step 2: Identify the Effect of Adding Argon
Argon is an inert gas, meaning it does not react with the components of the equilibrium. When argon is added to the system at constant volume, it increases the total pressure of the system without affecting the partial pressures of the reactants and products.

**Hint:** Consider the properties of inert gases and how they interact with existing gases in a closed system.

### Step 3: Apply Le Chatelier's Principle
Le Chatelier's Principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change. However, since argon is inert and does not affect the concentrations of \( N_2 \), \( H_2 \), or \( NH_3 \), the equilibrium position will not shift.

**Hint:** Recall how Le Chatelier's Principle applies to changes in concentration and pressure.

### Step 4: Analyze the Concentrations
At constant volume, the addition of argon does not change the concentrations of the reactants and products because the volume remains the same. The partial pressures of \( N_2 \), \( H_2 \), and \( NH_3 \) remain unchanged.

**Hint:** Think about how concentration is defined and how it relates to volume and moles.

### Step 5: Conclusion
Since the addition of argon at constant volume does not change the concentrations of the reactants and products, there will be no shift in the equilibrium position. Therefore, the correct answer is that the equilibrium will not shift in any direction.

**Final Answer:** The equilibrium will not shift in any direction.