Le chatelier principal- concentration change
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In the late 1800's, French chemist Henri-Louis Le Châtelier discovered that if a stress is applied to a system at equilibrium, the system will shift in a direction to try to relieve some of the stress. This is known as Le Châtelier principle. In this lesson, we will look at how changes in concentration of reactants and products affect chemical equilibrium.
Suppose we have a reaction at equilibrium and the concentration of one of the reactants is increased. According to Le Châtelier's principle, as a result of this stress, more collision will occur between reactants resulting in more products being formed. We refer to this as a shift to the right (in other words, the equilibrium is shifted in the direction of more products being formed).
Alternatively, if we were to remove product from a reaction at equilibrium, thereby decreasing the concentration of a product, again, the system would adjust to relieve this stress by forming more product (working to replace what had been removed), and thereby, again, shifting the reaction to the right.
If, on the other hand, we were to add product to the reaction, this would shift the reaction to the left, meaning that the stress would be relieved by converting some of the product back into reactants.
Indicate whether Le Châtelier's principle predicts a shift to the left (forming more reactants) or to the right (forming more products) for each of the following changes made to a system in equilibrium.
1. Addition of a reactant
2. Removal of a product
3. Addition of a product
4. Removal of a reactant