CHEM 404 Lecture 10: Introduction to Equilibrium
Document Summary
Reactions more often than not do not go in one direction only. Instead, products can collide with each other, and re-form the reactants: reactants are never completely used up. Reaction can achieve balance by balancing the rates of forward and backward reactions. When a reaction begins, the rate of the forward reaction is high. The concentration of product increases since forward reaction is fast. At first, there is little or no product, so the reaction can"t really go backwards yet. Over time, as product builds up, the rate of the backward reaction increases. At equilibrium: rates of the forward and backward reactions are equal, concentrations are stable: as fast as product is made, reactant is reformed. At first: reaction seems to go in one direction after dotted line, reaction reaches equilibrium (notice the concentrations don"t change anymore) Reminder: in a stoppered flask, evaporation and condensation will eventually come to equilibrium.
