To determine the direction in which the reaction shifts when more [tex]\( I_2 \)[/tex] is added, we can use Le Chatelier's Principle. Le Chatelier's Principle states that if a dynamic equilibrium system is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
The given chemical reaction is:
[tex]\[ 51.8 \text{ kJ} + H_2(g) + I_2(g) \rightleftharpoons 2 HI(g) \][/tex]
We need to analyze what happens when more [tex]\( I_2 \)[/tex] is added.
### Step-by-Step Solution:
1. Identify the disturbance:
Additional [tex]\( I_2 \)[/tex] is introduced to the system. This increases the concentration of [tex]\( I_2 \)[/tex] on the reactant side.
2. Apply Le Chatelier's Principle:
According to the principle, the system will try to counteract this change. Since the concentration of a reactant has been increased, the system will shift in the direction that consumes [tex]\( I_2 \)[/tex].
3. Determine the direction of the shift:
The reaction will shift towards the products (to the right) to consume the added [tex]\( I_2 \)[/tex]. This would be the direction that reduces the concentration of [tex]\( I_2 \)[/tex] by forming more [tex]\( HI \)[/tex].
By following these steps, we conclude that when more [tex]\( I_2 \)[/tex] is added to the reaction mixture, the equilibrium will shift to the right, towards the production of more [tex]\( HI \)[/tex].
### Conclusion:
The reaction shifts to the right, or towards the products.
Correct Answer:
A. The reaction shifts right or to products.
