When considering how a system at equilibrium responds to changes, we can use Le Chatelier's principle. This principle states that if a change is imposed on a system at equilibrium, the system will shift in the direction that counteracts the change.
In the given equilibrium reaction:
[tex]\[ 2 SO_2(g) + O_2(g) \rightleftharpoons 2 SO_3(g) + 198 \text{ kJ} \][/tex]
we are adding more [tex]\( SO_3 \)[/tex] gas to the system. Let's analyze the situation step-by-step:
1. According to Le Chatelier's principle, the addition of [tex]\( SO_3 \)[/tex] to the system increases the concentration of [tex]\( SO_3 \)[/tex].
2. The system will try to counteract this increase in [tex]\( SO_3 \)[/tex] concentration. To do that, it will shift the equilibrium position to the left (towards the reactants).
3. Shifting the equilibrium to the left means that [tex]\( SO_3 \)[/tex] will decompose into [tex]\( SO_2 \)[/tex] and [tex]\( O_2 \)[/tex], in order to decrease the concentration of [tex]\( SO_3 \)[/tex].
Therefore, as a result of adding [tex]\( SO_3 \)[/tex] to the system:
- The reaction will shift toward the reactants (left).
- The concentrations of [tex]\( SO_2 \)[/tex] and [tex]\( O_2 \)[/tex] will increase.
Hence, the correct change for the system is:
"The reaction will shift toward the reactants (left) and increase the concentrations of [tex]\( SO_2 \)[/tex] and [tex]\( O_2 \)[/tex]."
