Final answer:
When an equilibrium strongly favors products, there is a greater concentration of products than reactants. This can be indicated by a shift to the right, a shift to the product side, or a strong favoring of the forward reaction.
Step-by-step explanation:
When an equilibrium strongly favors products, it means that there is a greater concentration of products than reactants at equilibrium. This can be indicated by a shift of the equilibrium to the right, a shift to the product side, or a strong favoring of the forward reaction.
For example, if the equilibrium constant (K) is greater than 1, it indicates that products predominate at equilibrium. Chemists say that the equilibrium lies to the right as written, favoring the formation of products.
In contrast, if K is less than 1, it indicates that reactants predominate at equilibrium, and the equilibrium lies to the left as written, favoring the formation of reactants.