Certainly! Let's analyze the provided chemical system and the changes occurring when some [tex]\(O_2\)[/tex] gas is removed from the container.
The balanced chemical equation is:
[tex]\[ 2 \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \text{SO}_3(g) + 198\ \text{kJ} \][/tex]
This reaction is at equilibrium initially.
When a system at equilibrium experiences a change in concentration, pressure, or temperature, it will shift in a direction that counteracts the change. This principle is known as Le Chatelier's Principle.
In this scenario, [tex]\(O_2\)[/tex] gas is removed from the system. Let's analyze what happens step-by-step:
1. Change in Concentration:
- The removal of [tex]\(O_2\)[/tex] decreases its concentration in the system.
2. Applying Le Chatelier's Principle:
- According to Le Chatelier's Principle, the system will try to counteract the decrease in [tex]\(O_2\)[/tex] concentration.
- To do this, the reaction will shift in a direction that produces more [tex]\(O_2\)[/tex].
3. Direction of the Shift:
- In the given reaction:
[tex]\[ 2 \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \text{SO}_3(g) + 198\ \text{kJ} \][/tex]
- By shifting to the left (toward the reactants), the reaction will produce more [tex]\(O_2\)[/tex].
4. Impact on Concentrations:
- Shifting toward the reactants means converting some of the [tex]\(SO_3\)[/tex] back into [tex]\(SO_2\)[/tex] and [tex]\(O_2\)[/tex].
- As a result, the concentration of [tex]\(SO_2\)[/tex] will increase.
- The concentration of [tex]\(SO_3\)[/tex] will decrease.
Based on this analysis, the correct change that will occur in the system is:
The reaction will shift toward the reactants (left) and increase the concentration of SO
