Let's match each action to its effect on the equilibrium position for the reaction [tex]\( N_{2(g)} + 3 H_{2(g)} \rightleftharpoons 2 NH_{3(g)} \)[/tex]. Here's the detailed reasoning for each action:
### 1. Removing Ammonia
Removing ammonia from the reaction mixture reduces the concentration of one of the products. According to Le Chatelier's Principle, the equilibrium will shift in the direction that opposes this change, i.e., it will produce more ammonia to replace the removed ammonia. Therefore, removing ammonia shifts the equilibrium to the right.
Match: Removing ammonia - Shift to the right (C)
### 2. Removing Hydrogen Gas
Removing hydrogen gas from the reaction mixture reduces the concentration of one of the reactants. According to Le Chatelier's Principle, the equilibrium will shift in the direction that opposes this change, i.e., it will produce more hydrogen gas to replace the removed hydrogen. This shift will favor the decomposition of ammonia back into nitrogen and hydrogen gas. Therefore, removing hydrogen gas shifts the equilibrium to the left.
Match: Removing hydrogen gas - Shift to the left (B)
### 3. Adding a Catalyst
Adding a catalyst to a reaction speeds up the rate at which the reaction reaches equilibrium but does not change the position of the equilibrium itself. A catalyst provides an alternative pathway with a lower activation energy for both the forward and reverse reactions, thereby increasing the rate of both reactions equally. Hence, adding a catalyst has no effect on the equilibrium position.
Match: Adding a catalyst - No effect (A)
Based on this reasoning, the matches for each action to its effect on the equilibrium position are:
- Removing ammonia: [tex]\(C\)[/tex]
- Removing hydrogen gas: [tex]\(B\)[/tex]
- Adding a catalyst: [tex]\(A\)[/tex]
This translates to:
```
('C', 'B', 'A')
```
