Addition of inert gas to system
`N_(2)(g) + 3H_(2)(g) at equillibrium at constant volume. Then

Options

A. `N_2 and H_2` are formed in abundance
B. `N_2, H_2 and NH_3` will have the same molar concentration
C. The production of ammonia increases
D. No change in the equilibrium

Answer

To solve the problem regarding the addition of an inert gas to the equilibrium system \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \) at constant volume, we can follow these steps:

### Step 1: Understand the System
We are given a chemical equilibrium involving nitrogen gas, hydrogen gas, and ammonia gas. The reaction is:
\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]

### Step 2: Identify the Effect of Adding Inert Gas
When an inert gas is added to the system at constant volume, it does not react with any of the components of the equilibrium. The total pressure of the system will increase due to the addition of the inert gas, but the concentration of the reactants and products will remain unchanged.

### Step 3: Concentration Calculation
Concentration is defined as the number of moles of a substance per unit volume. Since we are adding an inert gas at constant volume, the moles of \( N_2 \), \( H_2 \), and \( NH_3 \) remain the same, and thus their concentrations do not change.

### Step 4: Apply Le Chatelier's Principle
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change (like pressure change), the equilibrium will shift in a direction that counteracts that change. However, since the concentrations of the reactants and products remain constant (as established in Step 3), there is no disturbance to the equilibrium position.

### Step 5: Conclusion on Equilibrium Position
Since the addition of the inert gas does not change the concentrations of the reactants and products, the position of equilibrium remains unaffected. Therefore, the correct conclusion is that there is no change in the equilibrium.

### Final Answer
The correct option is that there is no change in equilibrium.

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