On increasing the pressure, in which dirction will the gas phase reaction proceed to re-establish equilibrium, is predicated by applying the Le Chatelier's principle. Consider the reaction.
`N_(2)(g)+3H_(2)hArr 2NH_(3)(g)`
Which of the following is correct, if the total pressure at which the equlibrium is established, is increased without changing the temperature ?

Options

A. K will remain same.
B. K will decrease.
C. K will increase.
D. K will increase initially and decrease when pressure is very high.

Explanation

To solve the question regarding the effect of increasing pressure on the equilibrium of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \), we can apply Le Chatelier's principle. Here’s a step-by-step breakdown of the solution:

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

### Step 2: Count the Moles of Gas
Next, we need to count the number of moles of gas on both sides of the reaction:
- On the left side (reactants): 1 mole of \( N_2 \) + 3 moles of \( H_2 \) = **4 moles**
- On the right side (products): 2 moles of \( NH_3 \) = **2 moles**

### Step 3: Apply Le Chatelier's Principle
Le Chatelier's principle states that if a system at equilibrium is subjected to a change in pressure, the equilibrium will shift in the direction that reduces the pressure. This means that the system will shift towards the side with fewer moles of gas.

### Step 4: Determine the Direction of Shift
Since there are 4 moles of gas on the reactants' side and only 2 moles on the products' side, increasing the pressure will shift the equilibrium to the right, towards the production of \( NH_3 \).

### Conclusion
Thus, when the total pressure at which the equilibrium is established is increased, the equilibrium will shift to the right, favoring the formation of ammonia (\( NH_3 \)).

### Final Answer
The correct direction of the shift in equilibrium upon increasing pressure is towards the products side, which is the formation of \( NH_3 \).

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