5 posts • Page 1 of 1
When calculating the reaction quotient you are evaluating the reaction at some time that is not at equilibrium and you use the value to determine its relativity to reaching equilibrium. In the case where Q < K, there are more reactants compared to the reaction at equilibrium, therefore more products need to be created, hence the forward reaction is favored. Vice versa when Q > K, more products are present therefore reactants need to be made and the reverse reaction is favored.
Who is online
Users browsing this forum: No registered users and 0 guests