To determine the effect of adding more [tex]\( Na_2O_2 \)[/tex] to the system at equilibrium, we can use Le Chatelier's principle. Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
The reaction given is:
[tex]\[
2 Na(s) + O_2(g) \rightleftharpoons Na_2O_2(s)
\][/tex]
We are specifically interested in the effect of adding more [tex]\( Na_2O_2 \)[/tex], the product of this reaction. Let's go through the steps:
1. Identify the disturbance:
We are adding more [tex]\( Na_2O_2 \)[/tex], which increases the concentration of the solid product.
2. Apply Le Chatelier's principle:
According to Le Chatelier's principle, the system will respond to this disturbance by shifting the equilibrium position to reduce the effect of the added [tex]\( Na_2O_2 \)[/tex]. This means that the system will try to consume some of the added [tex]\( Na_2O_2 \)[/tex] to restore equilibrium.
3. Determine the direction of the shift:
To consume the added [tex]\( Na_2O_2 \)[/tex], the equilibrium will shift towards the left (the reverse reaction). This shift will produce more [tex]\( Na \)[/tex] and [tex]\( O_2 \)[/tex] from the breakdown of [tex]\( Na_2O_2 \)[/tex].
Therefore, the equilibrium position will shift to produce more [tex]\( Na \)[/tex] and [tex]\( O_2 \)[/tex].
The correct answer is:
A. The equilibrium position would shift to produce more [tex]\( Na \)[/tex] and [tex]\( O_2 \)[/tex].
