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Dynamic Equilibrium
A state in which the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products over time.
Le Chatelier's Principle
States that when a system at equilibrium is subjected to a change, it will adjust to counteract the change and establish a new equilibrium.
Factors Affecting Equilibrium
Concentration, temperature, and pressure are factors that can affect the equilibrium position of a chemical reaction.
Equilibrium Constant (Kc)
A quantitative measure of the position of equilibrium, calculated by taking the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients.
Equilibria in Solutions
Equilibria involving solutions, where the concentrations of solutes are expressed in terms of molarity.
Energy Profiles of Reversible Reactions
Graphical representations that show the energy changes that occur during a reversible reaction, indicating the activation energy and the energy difference between the reactants and products.
Calculating Equilibrium Concentrations
A step-by-step guide on how to calculate the concentrations of reactants and products at equilibrium using the equilibrium constant and initial concentrations.
Industrial Processes
Case studies of industrial processes, such as the Haber process and the Contact process, that utilize chemical equilibrium to optimize yield and efficiency.
Laboratory Experiments
Practical experiments conducted in the laboratory to observe and study changes in equilibrium, following safety guidelines and procedures.
Chemical equilibrium
A state where reactants and products are continuously interconverted.
Equilibrium constant (Kc)
The ratio of product concentrations to reactant concentrations at equilibrium.
Le Chatelier's principle
The equilibrium position can be manipulated by changing the temperature, pressure, or concentration.
Effect of concentration changes on equilibrium
Shifts the equilibrium towards the side with fewer moles of the added substance or towards the side with more moles of the removed substance.
Effect of pressure changes on equilibrium
Changes in pressure only affect equilibrium if there is a difference in the number of moles of gas on each side of the reaction.
Effect of temperature changes on equilibrium
Increasing temperature favors the endothermic reaction, while decreasing temperature favors the exothermic reaction.
Equilibrium constant calculations
The process of determining the numerical value of the equilibrium constant for a chemical reaction based on the concentrations of reactants and products at equilibrium.
Equilibrium shift predictions
The ability to predict the direction in which an equilibrium will shift when certain changes are made to the system, such as changes in temperature, pressure, or concentration.
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