equilibria

• Chemical Equilibria are reversible reactions where the products can react to reform the original reactants.
• Le Chaterlier's Principle states that if a chemical change occurs during a reaction, the direction of the reaction will change.
• The Equilibrium Constant is a measure of the strength of a chemical reaction and is calculated using the formula K = [Products] / [Reactants].
• Changes Affecting the Equilibrium Constant include temperature, concentration, and pH.
• Industrial Processes involve chemical reactions used in various industries.
• Acids & Bases are a topic in Chemistry that involves understanding the properties and reactions of these substances.
• Brønsted–Lowry Theory is a concept in Chemistry that explains the properties and reactions of acids and bases.
• Acid & Base Dissociation is a concept in Chemistry that explains how acids and bases dissociate into ions.
• pH Scale is a tool used in Chemistry to measure the acidity or alkalinity of a solution.
• Strength of Acids & Bases is a topic in Chemistry that involves understanding the strength of acids and bases.
• pH T itration Curves are a tool used in Chemistry to measure the strength of acids and bases.
• The Brønsted-Lowry Theory defines acids and bases in terms of proton transfer between chemical compounds.
• A Brønsted-Lowry acid is a species that gives away a proton (H).
• Water acts as a Brønsted-Lowry acid when it donates a proton to ammonia which accepts the proton using its lone pair of electrons.
• Water acts as a Brønsted-Lowry base when it accepts a proton from hydrochloric acid using its lone pair of electrons.
• Species that can act both as acids and bases are called amphoteric.
• A Brønsted-Lowry base is a species that accepts a proton (H) using its lone pair of electrons.
• When hydrogen loses an electron to become H only a proton remains, which is why a H ion is also called a proton.
• The diagram shows a Brønsted-Lowry acid which donates the proton to the Brønsted-Lowry base that accepts the proton using its lone pair of electrons.
• The Brønsted-Lowry Theory is not limited to aqueous solutions only and can also be applied to reactions that occur in the gas phase.
• An atom of hydrogen contains 1 proton, 1 electron and 0 neutrons.
• Indicators used in T itration are a tool used in Chemistry to measure the strength of acids and bases.
• The concentrations of the reactants and products in a chemical reaction do not remain constant at dynamic equilibrium, but they remain constant.
• If the position of equilibrium in a chemical reaction shifts to the left, it means the concentration of reactants increases.
• The reaction will absorb the excess energy and since the forward reaction is endothermic, the equilibrium will shift to the right.
• The concentrations of the reactants and products in a chemical reaction will change as the reaction progresses, only until the equilibrium is reached.
• The position of the equilibrium in a chemical reaction refers to the relative amounts of products and reactants in an equilibrium mixture.
• Changes in concentration can affect the position of the equilibrium in a chemical reaction.
• Le Chatelier’s principle is used to predict changes to the position of equilibrium when there are changes in temperature, pressure or concentration.
• The effects of concentration can be seen in a table.
• Le Chatelier’s principle states that if a change is made to a system at dynamic equilibrium, the position of the equilibrium moves to minimise this change.
• If the position of equilibrium in a chemical reaction shifts to the right, it means the concentration of products increases.
• Changes in temperature can affect the position of the equilibrium in a chemical reaction.
• Changes in pressure only affect reactions where the reactants or products are gases.
• Changes in pressure can affect the position of the equilibrium in a chemical reaction.
• The equilibrium expression is an expression that links the equilibrium constant, K, to the concentrations of reactants and products at equilibrium taking the stoichiometry of the equation into account.
• The equation to calculate the total pressure in a mixture of gases is: p = p1 + p2 + p3 + ...
• The total pressure is the sum of the partial pressure.
• To calculate the partial pressures of each gas, the following relationship can be used: p1/p2/p3/... = x/y/z/... where x, y, z are the mole fractions of each gas.
• The reaction will absorb the excess energy and since this causes a shift of the equilibrium towards the right (as more CO (g) is formed) this means that the reaction is endothermic (because endothermic reactions favour the products).