Equilibria

🔬 Chapter 8: Equilibrium 🔬Learning Outcomes 🎯:Explain what is meant by a reversible reaction and dynamic equilibrium.State Le Chatelier’s principle and apply it to deduce qualitatively the effect of changes in temperature, concentration, or pressure on a system at equilibrium.State whether changes in temperature, concentration, or pressure or the presence of a catalyst affect the value of the equilibrium constant for a reaction.Deduce expressions for equilibrium constants in terms of concentrations (Kc) and partial pressures (Kp).Calculate the value of equilibrium constants in terms of concentrations or partial pressures and the quantities of substances present at equilibrium.Describe and explain the conditions used in the Haber process and the Contact process.Show understanding of, and use, the Brønsted–Lowry theory of acids and bases.Explain qualitatively the differences in behavior between strong and weak acids and bases and the pH values of their aqueous solutions in terms of the extent of dissociation.Reversible Reactions and Dynamic Equilibrium 🔄:A reversible reaction is one in which the products can change back to reactants.Chemical equilibrium is dynamic because the backward and forward reactions are both occurring at the same time.A chemical equilibrium is reached when the rates of the forward and reverse reactions are equal.Le Chatelier’s Principle 📊:Le Chatelier’s principle states that when the conditions in a chemical equilibrium change, the position of equilibrium shifts to oppose the change.Changes in temperature, pressure, and concentration of reactants and products affect the position of equilibrium.Equilibrium Constants (Kc and Kp) 🧮:For an equilibrium reaction, there is a relationship between the concentrations of the reactants and products which is given by the equilibrium constant K.Equilibrium constants in terms of concentrations (Kc) and partial pressures (Kp) can be deduced from appropriate data.Brønsted–Lowry Theory of Acids and Bases 🧪:The Brønsted–Lowry theory of acids and bases states that acids are proton donors and bases are proton acceptors.Strong acids and bases are completely ionized in aqueous solution whereas weak acids and bases are only slightly ionized.Strong and weak acids and bases can be distinguished by the pH values of their aqueous solutions.🔍