Final answer:
Chemical reactions like the synthesis of ammonia may shift towards reactants or products depending on changes in reaction conditions, which can be understood through Le Chatelier's principle. Factors like adding or removing a reactant or product, and stoichiometry play key roles in predicting the shift's direction.
Step-by-step explanation:
When considering shifts in chemical reactions, such as the synthesis of ammonia (NH3) from nitrogen (N2) and hydrogen (H2), the concept of equilibrium and Le Chatelier's principle come into play. The reaction N2 + 3H2 → 2NH3 can shift either toward the reactants or toward the products in response to external changes.
- If additional H2 is introduced into the system, the reaction will shift toward the products to reduce the concentration of the added reactant.
- If more NH3 is added to the system, the reaction shifts toward the reactants to decrease the concentration of the added products.
- Conversely, if NH3 is removed, the reaction shifts toward the products to replace the NH3 that has been taken away.
It's critical to consider both stoichiometry and limiting reactants when evaluating such changes in equilibrium.