At constant pressure, the addition of argon in Haber's process

Options

A. Reduces the formation of ammonia from `N_(2)andH_(2)`
B. Increases the formation of ammonia from `N_(2)and H_(2)`
C. Does not affect the equlibrium of the reaction in which ammonia is formed from `N_(2)and H_(2)`
D. Reduces the dissociation of ammonia

Answer

To solve the question regarding the effect of adding argon gas at constant pressure in the Haber process, we can follow these steps:

### Step 1: Understand the Haber Process
The Haber process is a chemical reaction used to synthesize ammonia (NH3) from nitrogen (N2) and hydrogen (H2). The balanced equation for this reaction is:

\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]

### Step 2: Identify the Moles of Gases
In the balanced equation, we have:
- Reactants: 1 mole of N2 + 3 moles of H2 = 4 moles of gas
- Products: 2 moles of NH3

### Step 3: Consider the Effect of Adding Argon
Argon is an inert gas, meaning it does not react with the other gases in the reaction. When argon is added at constant pressure, it increases the total number of gas molecules in the system. However, since the pressure is held constant, the volume of the system must change.

### Step 4: Apply Le Chatelier's Principle
According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in conditions (such as pressure or volume), the equilibrium will shift in a direction that counteracts that change.

In this case, since we are effectively decreasing the volume (to maintain constant pressure with the addition of argon), the equilibrium will shift toward the side with fewer moles of gas to minimize the change.

### Step 5: Determine the Direction of the Shift
In our reaction:
- The reactants side has 4 moles of gas.
- The products side has 2 moles of gas.

Since the addition of argon (an inert gas) leads to a decrease in volume, the equilibrium will shift to the left (toward the reactants) to reduce the number of gas moles.

### Step 6: Conclusion
As a result, the addition of argon gas reduces the formation of ammonia from nitrogen and hydrogen. Therefore, the correct option is:

**Option 1: Reduces the formation of ammonia from N2 and H2.**

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