When we analyze how a change affects a system at equilibrium, we apply Le Chatelier's Principle. This principle states that if a change is made to a system at equilibrium, the system will respond in a way that counteracts the change and re-establishes equilibrium.
Here, we consider the reaction:
[tex]\[ 2 H_2 + O_2 \rightleftharpoons 2 H_2O \][/tex]
If more [tex]\( O_2 \)[/tex] (oxygen) is added to this reaction at equilibrium, let's analyze what will happen:
1. The equilibrium will shift: According to Le Chatelier's Principle, the equilibrium will shift in the direction that consumes the added component. In this case, adding more [tex]\( O_2 \)[/tex] will shift the equilibrium to the right, favoring the production of [tex]\( H_2O \)[/tex] (water). This is because the system seeks to reduce the disturbance caused by the added [tex]\( O_2 \)[/tex].
So, option A is correct: "The equilibrium will shift to favor the production of [tex]\( H_2O \)[/tex]."
2. Reaction rates: When more [tex]\( O_2 \)[/tex] is added, the rate of the forward reaction will also increase because there is a higher concentration of one of the reactants ([tex]\( O_2 \)[/tex]). This increased rate will lead to a faster production of [tex]\( H_2O \)[/tex].
The rate of the forward reaction (where [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex] react to form [tex]\( H_2O \)[/tex]) will increase because the system is responding to the increased availability of [tex]\( O_2 \)[/tex].
Therefore, option D is correct: "The rate at which [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex] react will increase."
### Conclusion:
The correct events that will happen when more [tex]\( O_2 \)[/tex] is added to this equilibrium reaction are:
- The equilibrium will shift to favor the production of [tex]\( H_2O \)[/tex]. (Option A)
- The rate at which [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex] react will increase. (Option D)
