A reaction quotient is the ratio between the concentration of products to the concentration of reactants at any point of the reaction. This means that the point when a reaction quotient is measured does not guarantee that the reaction is in equilibrium.
On the other hand, an equilibrium constant is the ratio between the concentration of products to the concentration of reactants at the equilibrium point. This means that when the ratio between reactants and products in a reaction reaches the equilibrium constant, the reaction is in equilibrium.
Figuring out the reaction quotient is very useful because you can figure out:
i) Whether the reaction is in equilibrium. (The reaction is in equilibrium if Q=K)
ii) If not, which direction would the reaction move.
--> If Q>K, it means that the reaction has more products than the equilibrium point. Hence, to reach the equilibrium point, the reaction would lose products, meaning that there would be a net reverse flow of reaction.
--> If K>Q, it means that the reaction has more reactants than the equilibrium point. Hence, to reach the equilibrium point, the reaction would lose reactants to produce more products, meaning that there would be a net forward flow of reaction.
Hi, thank you for your question.
A reaction quotient is the ratio between the concentration of products to the concentration of reactants at any point of the reaction. This means that the point when a reaction quotient is measured does not guarantee that the reaction is in equilibrium.
On the other hand, an equilibrium constant is the ratio between the concentration of products to the concentration of reactants at the equilibrium point. This means that when the ratio between reactants and products in a reaction reaches the equilibrium constant, the reaction is in equilibrium.
Does this answer your question?