Chemical Equilibrium | Le Chatelier's principle, Kc, Kp expressions

In many chemical processes, reactants do not completely turn into products. Instead, the reaction can move in both directions. This lesson covers the specific mechanics of reversible reactions, how they reach a state of dynamic balance, and how to mathematically calculate the equilibrium position. Here is the specific content covered in this lesson: • Reversible vs. Irreversible Reactions: Understanding the difference between one-way reactions and those where products can react to reform the original reactants. • The Concept of Dynamic Equilibrium: Explaining how a closed system reaches equilibrium when the rate of the forward reaction equals the rate of the reverse reaction, causing the concentrations of reactants and products to remain constant. • Le Chatelier’s Principle: The core rule stating that if a system at equilibrium is subjected to a change, the system will shift its position to counteract that change. We look at the specific effects of: • Concentration shifts • Temperature changes (endothermic vs. exothermic processes) • Pressure/Volume adjustments (gaseous systems) • The addition of a catalyst (and why it does not alter the equilibrium position) • The Equilibrium Constant (K_c): How to write the equilibrium law expression from a balanced chemical equation and perform standard calculations using product and reactant concentrations. #Chemistry #ChemicalEquilibrium #LeChatelier #ReversibleReactions #EquilibriumConstant #HighSchoolChemistry #STEM