Chemical equilibrium

This chapter analyses the reaction that ensues when reactants are mixed until equilibrium is established. It defines the term 'dynamic equilibrium', which refers to the fact that once equilibrium has been established, both forward and backward reactions continue at the same rate. It also talks about the presence of both reactants and products. Here, there is no further tendency for the mixture to undergo net change. The chapter cites the reaction between hydrogen and iodine to produce hydrogen iodide as an example. The chapter highlights how the equilibrium process may be investigated by setting up a reaction mixture of hydrogen and iodine in a sealed vessel, allowing it to come to equilibrium. It examines the ratio of reactants to products found at equilibrium. This is determined by the equilibrium constant for the reaction.