To analyze the effect of adding water ([tex]\(H_2O\)[/tex]) to the reaction
[tex]\[
\left( NH_4\right)_2CO_3(s) \rightleftharpoons 2 NH_3(g) + CO_2(g) + H_2O(g)
\][/tex]
we need to consider Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change.
When water is added to this reaction mixture, the concentration of [tex]\(H_2O(g)\)[/tex] on the product side increases. According to Le Chatelier's principle, the system will try to decrease the concentration of [tex]\(H_2O(g)\)[/tex] by shifting the equilibrium position to the left. This shift is a way for the system to reduce the disturbance caused by the added water.
As the equilibrium shifts to the left:
- More [tex]\((NH_4)_2CO_3(s)\)[/tex] will be formed.
- The concentrations of the products [tex]\(NH_3(g)\)[/tex] and [tex]\(CO_2(g)\)[/tex] will decrease over time because the reaction favors the formation of the solid reactant.
Therefore, the detailed effect of adding water to the reaction mixture is as follows:
Effect over time:
- The equilibrium will shift to the left.
- There will be increased formation of [tex]\((NH_4)_2CO_3(s)\)[/tex].
- The concentrations of [tex]\(NH_3(g)\)[/tex] and [tex]\(CO_2(g)\)[/tex] will decrease.
This response is consistent with Le Chatelier's principle, demonstrating how the system counteracts the addition of extra water by promoting the formation of the solid reactant, thus reducing the concentrations of the gaseous products.
