According to Le Chatelier's principle, does the equilibrium shift to the products or reactants when O2 is added to the equilibrium mixture of the following:
A. 302(g) - 2O3(g)
The reaction tries to undo what we've done; i.e., we add O2 so the reaction uses the extra O2 and the only way it can do that is to shift to the right toward the products.
According to Le Chatelier's principle, if O2 is added to the equilibrium mixture of the reaction 3O2(g) ⇌ 2O3(g), the equilibrium will shift towards the products.
To determine how the addition of O2 to the equilibrium mixture will affect the equilibrium, we can use Le Chatelier's principle. Le Chatelier's principle states that when a system at equilibrium is subjected to a change, it will respond in a way that counteracts the change.
In this case, O2 is being added to the equilibrium mixture of the reaction 3O2(g) ⇌ 2O3(g). According to Le Chatelier's principle, the system will respond by shifting the equilibrium in a direction that minimizes the effect of adding O2.
To analyze this, we need to consider the stoichiometry of the reaction. Since there are more moles of O2 on the reactant side compared to the product side, adding more O2 will cause the reactant side to have an excess of moles. As a result, the system will shift in the direction that consumes some of the excess reactant (O2). In other words, it will shift towards the products to try and reduce the excess O2 and restore equilibrium.
Therefore, according to Le Chatelier's principle, the equilibrium will shift to the right (towards the products) when O2 is added to the equilibrium mixture of the reaction 3O2(g) ⇌ 2O3(g).