If the concentration of a reactant is increased in a system at equilibrium, what

If the concentration of a reactant is increased in a system at equilibrium, what will happen according to Le Chatelier's principle?

If the concentration of a reactant is increased in a system at equilibrium, what will happen according to Le Chatelier's principle?

Step 1: Understand that a system at equilibrium means the forward and reverse reactions are happening at the same rate.
Step 2: Know that Le Chatelier's principle states that if you change something in the system, it will try to counteract that change.
Step 3: Recognize that increasing the concentration of a reactant means there are more reactant molecules available.
Step 4: Realize that to counteract the increase in reactant concentration, the system will try to use up some of the extra reactants.
Step 5: Understand that this will shift the equilibrium position to the right, which means more products will be formed.

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