Chemical equilibrium is a state in which the forward and reverse reactions in a chemical system occur at equal rates, resulting in no overall change in the concentrations of reactants and products.
One way to demonstrate chemical equilibrium is by using a reaction that produces a visible color change, such as the reaction between iron(III) chloride and potassium thiocyanate. As the reaction reaches equilibrium, the color will remain constant, indicating that the forward and reverse reactions are occurring at equal rates.
Some common chemical equilibrium experiments for a high school classroom include the reaction between iron(III) chloride and potassium thiocyanate, the reaction between cobalt(II) chloride and hydrochloric acid, and the reaction between silver nitrate and potassium chromate.
It is important to wear appropriate personal protective equipment, such as goggles and gloves, when conducting chemical equilibrium experiments. Students should also be reminded to follow proper lab safety protocols, such as not eating or drinking in the lab and washing their hands after handling chemicals.
Chemical equilibrium is a fundamental concept in many industrial processes, such as the production of fertilizers and the synthesis of pharmaceuticals. By understanding chemical equilibrium, students can better understand and appreciate the real-world applications of chemistry.