For the equilibrium at 2.0 bar `N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g)) ` , what happens to the equillibrium when pressure increased

Answer

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 will follow these steps:

### Step 1: Identify the reaction and its components
The reaction involves nitrogen gas (N₂), hydrogen gas (H₂), and ammonia gas (NH₃). The balanced equation shows that 1 mole of nitrogen and 3 moles of hydrogen react to form 2 moles of ammonia.

### Step 2: Count the number of moles of gases on both sides
- **Reactants side**:
- 1 mole of N₂ + 3 moles of H₂ = 4 moles of gas
- **Products side**:
- 2 moles of NH₃

### 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 counteracts the change. In this case, increasing the pressure will favor the side with fewer moles of gas.

### Step 4: Determine the direction of the shift
Since there are 4 moles of gas on the reactants side and only 2 moles of gas on the products side, increasing the pressure will shift the equilibrium towards the products side (right side), where there are fewer moles of gas.

### Step 5: Conclusion
Thus, when the pressure is increased, the equilibrium will shift to the right, favoring the formation of ammonia (NH₃).

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