To determine the correct answer for the effect of adding water ([tex]\(H_2O\)[/tex]) on the reaction
[tex]\[
\left( NH_4 \right)_2 CO_3(s) \rightleftharpoons 2 NH_3(g) + CO_2(g) + H_2O(g),
\][/tex]
we need to understand the principle of chemical equilibrium, specifically Le Chatelier's Principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
Here, water ([tex]\(H_2O\)[/tex]) is one of the products in the reaction. If we add more [tex]\(H_2O\)[/tex], the system will adjust to counter the increase in [tex]\(H_2O\)[/tex] by shifting the equilibrium position to the left. This means the reaction will produce more reactants and fewer products.
Therefore:
- The concentration of products ([tex]\(NH_3(g)\)[/tex], [tex]\(CO_2(g)\)[/tex], and [tex]\(H_2O(g)\)[/tex]) would decrease.
- The concentration of reactants ([tex]\((NH_4)_2CO_3(s)\)[/tex]) would increase.
Given this information, the correct answer is:
C. The concentration of products would decrease, and the concentration of reactants would increase.
