* Equilibrium means the rates of the forward and reverse reactions are equal. This doesn't mean there are equal amounts of reactants and products, it just means the net change in their concentrations is zero.
* Equilibrium constant (K) is a measure of the relative amounts of reactants and products at equilibrium. A large K value indicates that the reaction favors the formation of products.
* Favoring products means that the reaction will proceed to a greater extent in the forward direction to form products, resulting in a higher concentration of products at equilibrium.
Here are some implications of a reaction system at equilibrium with mostly product:
* The change in Gibbs free energy (ΔG) is negative, indicating a spontaneous reaction.
* The reaction quotient (Q) is greater than the equilibrium constant (K), meaning the system is not at equilibrium and will shift to the left (toward reactants) to reach equilibrium.
In summary, a reaction system at equilibrium with mostly product is a highly favorable reaction that has proceeded to a significant extent to form products.
