Physical and chemical equilibrium can respond to a change in their pressure, temperature, and concentration of reactants and products. To describe the change in the equilibrium we have a principle named Le Chatelier principle. According to this principle, even if we make some changes in equilibrium, then also the system even re-establishes the equilibrium by undoing the effect.
In the reaction `N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)`. If we increase the pressure of the system, the equilibrium is

Options

A. Shifts in the product side
B. Shift un reactant side
C. Remains unchanged
D. Cannot be predicted

Explanation

To solve the question regarding the effect of increased pressure on the equilibrium of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \), we can follow these steps:

### Step 1: Identify the Reaction and Moles
The given reaction is:
\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]

Next, we need to count the number of moles of gas on both sides of the equation:
- **Reactants**: \( N_2(g) + 3H_2(g) \) = 1 + 3 = **4 moles**
- **Products**: \( 2NH_3(g) \) = **2 moles**

### Step 2: Apply Le Chatelier's Principle
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in pressure, the equilibrium will shift in the direction that reduces the pressure. This typically means shifting towards the side with fewer moles of gas.

### Step 3: Analyze the Effect of Increased Pressure
Since we have identified that there are 4 moles of gas on the reactant side and 2 moles of gas on the product side, increasing the pressure will favor the side with fewer moles of gas. In this case, the equilibrium will shift to the right (towards the products).

### Step 4: Conclusion
Therefore, when the pressure of the system is increased, the equilibrium will shift towards the product side, resulting in the formation of more ammonia (\( NH_3 \)).

### Final Answer
The equilibrium will shift to the right, favoring the production of ammonia (\( NH_3 \)).

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