Final answer:
To determine if a reaction is reactant-favored or product-favored, look at the equilibrium constant (K). If K is greater than 1, the reaction is product-favored; if less than 1, it's reactant-favored. Changes in reaction conditions will cause shifts in equilibrium in accordance with Le Châtelier's Principle.
Step-by-step explanation:
In chemistry, whether a reaction is reactant-favored or product-favored can be determined by the equilibrium constant (K). If the value of K is greater than 1, the reaction is typically product-favored, meaning that at equilibrium, there will be a higher concentration of products than reactants. Conversely, if the value of K is less than 1, the reaction is reactant-favored, indicating that the reactants predominate at equilibrium.
As a reaction heads towards equilibrium, the rates of the forward and reverse reactions change. Initially, the forward reaction rate is higher as the concentration of reactants is higher. As the reaction progresses and products begin to form, the rate of the forward reaction decreases while the rate of the reverse reaction increases.