How does concentration effect Le Chatelier's principle?

Question

Serenity Allen · Accepted Answer

Reactant or product concentration changes will result in a shift to restore equilibrium.

On the other hand, if a substance's concentration is lowered, the reaction will produce more of that substance until equilibrium is restored.

Ammonia is created through the reaction of nitrogen and hydrogen gases.

#N_2# + #3H_2# ----> 2 # NH_3#

Increases in either nitrogen or hydrogen gas concentration will result in the consumption of both reactants, which will tip the scales in favor of the product—a higher ammonia concentration.

Caleb Adams · Answer

undefined Concentration changes can affect Le Chatelier's principle by shifting the equilibrium of a chemical reaction towards the side with the fewer number of moles when the concentration of a reactant or product is changed. If the concentration of a reactant is increased, the equilibrium will shift to the right to consume the excess reactant, and vice versa. If the concentration of a product is increased, the equilibrium will shift to the left to produce more reactants, and vice versa.

Wyatt Adkins · Answer

undefined Changes in concentration can affect Le Chatelier's principle by shifting the equilibrium position of a chemical reaction. Specifically:

1. **Increasing Concentration**: Adding more reactants or products to a system at equilibrium will cause the system to shift in the direction that consumes or removes those substances to partially offset the change.

2. **Decreasing Concentration**: Removing reactants or products from a system at equilibrium will cause the system to shift in the direction that replaces or replenishes those substances to partially offset the change.

This shift occurs because the reaction will try to establish a new equilibrium position that reduces the stress caused by the concentration change, thereby obeying Le Chatelier's principle.