Grade 11 Kinetics And Equilibrium Essay
Unit 11: Kinetics and Equilibrium
Activated complex: an intermediate state that is formed during the conversion of reactants into products, the structure that results at the maximum energy point along the reaction path.
Activation energy: a chemical reaction is the difference between the energy of the activated complex and the energy of the reactants.
Catalyst: substance that increases the rate of a chemical reaction by reducing the activation energy, but which is left unchanged by the reaction.
Entropy: The measure of the disorder of a system, usually denoted by the letter S. A highly ordered system has low entropy.
Enthalpy: a thermodynamic property of a system. It reflects the capacity to do non-mechanical work and the capacity to release …show more content…
heat. Enthalpy is denoted as H; specific enthalpy denoted as h.
Equilibrium: the state of a reversible reaction where the forward reaction rate is equal to the reverse reaction's rate.
Chemical Equilibrium: the state of a chemical reaction when the concentrations of the products and reactants are unchanged over time.
Physical equilibrium: the equilibrium of the physical states of the same substance.
Equilibrium expression: may be expressed in terms of the concentration of the products and reactants.
Reversible reaction: a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
Effective collisions: a collision between two reactants with the correct orientation and with sufficient energy to overcome the activation energy barrier
Reaction rate: the rate at which the reactants of a chemical reaction form the products.
Le Chatelier’s Principle: the principle when a stress is applied to a chemical system at equilibrium, the equilibrium will shift to relieve the stress.
Potential energy diagram: plots the change in potential energy that occurs during a chemical reaction. This first video takes you through all the basic parts of the PE diagram.
Stress: changes in temperature, number of moles, or volume which cause as system to be disturbed from equilibrium
Elastic collisions: a collision in which the total kinetic energy of the colliding bodies or particles is the same after the collisionas it was before
Common ion effect: describes the suppressing effect on ionization of an electrolyte when when another electrolyte is added that shares a common
ion.
Reaction mechanism: is the step by step sequence of elementary reactions by which overall chemical change occurs
Gibbs free energy: a thermodynamic property that was defined in 1876 by Josiah Willard Gibbs to predict whether a process will occur spontaneously at constant temperature and pressure. Gibbs free energy G is defined as G = H - TS where H, T and S are the enthalpy, temperature, and entropy.
Reaction order: a given substance (such as reactant, catalyst or product) is defined as the index, or exponent, to which its concentration term in threat is raised.
Rate law: an equation that links the reaction rate with concentrations or pressures of reactants and constant parameters (normally rate coefficients and partial reaction orders).
Equilibrium constant: the ratio of the equilibrium concentrations of the products raised to the power of their stoichiometric coefficients to the equilibrium concentrations of the reactants raised to the power of their stoichiometric coefficients.
Spontaneous reactions: will occur without any energy input from the surroundings. A process that will occur on its own.
Inhibitor: a substance that delays, slows or prevents a chemical reaction.
First order: a chemical reaction in which the rate of reaction is directly proportional to the concentration of the reacting substance
Second order: a chemical reaction in which the rate of reaction is proportional to the concentration of each of two reacting molecules
Solubility product constant: the equilibrium constant for a chemical reaction in which a solid ionic compound dissolves to yield its ions in solution.
Hess’ Law: Law which states that the energy change in an overall chemical reaction is equal to the sum of the energy changes in the individual reactions comprising it.
Activated complex: an intermediate state that is formed during the conversion of reactants into products, the structure that results at the maximum energy point along the reaction path.
Activation energy: a chemical reaction is the difference between the energy of the activated complex and the energy of the reactants.
Catalyst: substance that increases the rate of a chemical reaction by reducing the activation energy, but which is left unchanged by the reaction.
Entropy: The measure of the disorder of a system, usually denoted by the letter S. A highly ordered system has low entropy.
Enthalpy: a thermodynamic property of a system. It reflects the capacity to do non-mechanical work and the capacity to release …show more content…
heat. Enthalpy is denoted as H; specific enthalpy denoted as h.
Equilibrium: the state of a reversible reaction where the forward reaction rate is equal to the reverse reaction's rate.
Chemical Equilibrium: the state of a chemical reaction when the concentrations of the products and reactants are unchanged over time.
Physical equilibrium: the equilibrium of the physical states of the same substance.
Equilibrium expression: may be expressed in terms of the concentration of the products and reactants.
Reversible reaction: a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
Effective collisions: a collision between two reactants with the correct orientation and with sufficient energy to overcome the activation energy barrier
Reaction rate: the rate at which the reactants of a chemical reaction form the products.
Le Chatelier’s Principle: the principle when a stress is applied to a chemical system at equilibrium, the equilibrium will shift to relieve the stress.
Potential energy diagram: plots the change in potential energy that occurs during a chemical reaction. This first video takes you through all the basic parts of the PE diagram.
Stress: changes in temperature, number of moles, or volume which cause as system to be disturbed from equilibrium
Elastic collisions: a collision in which the total kinetic energy of the colliding bodies or particles is the same after the collisionas it was before
Common ion effect: describes the suppressing effect on ionization of an electrolyte when when another electrolyte is added that shares a common
ion.
Reaction mechanism: is the step by step sequence of elementary reactions by which overall chemical change occurs
Gibbs free energy: a thermodynamic property that was defined in 1876 by Josiah Willard Gibbs to predict whether a process will occur spontaneously at constant temperature and pressure. Gibbs free energy G is defined as G = H - TS where H, T and S are the enthalpy, temperature, and entropy.
Reaction order: a given substance (such as reactant, catalyst or product) is defined as the index, or exponent, to which its concentration term in threat is raised.
Rate law: an equation that links the reaction rate with concentrations or pressures of reactants and constant parameters (normally rate coefficients and partial reaction orders).
Equilibrium constant: the ratio of the equilibrium concentrations of the products raised to the power of their stoichiometric coefficients to the equilibrium concentrations of the reactants raised to the power of their stoichiometric coefficients.
Spontaneous reactions: will occur without any energy input from the surroundings. A process that will occur on its own.
Inhibitor: a substance that delays, slows or prevents a chemical reaction.
First order: a chemical reaction in which the rate of reaction is directly proportional to the concentration of the reacting substance
Second order: a chemical reaction in which the rate of reaction is proportional to the concentration of each of two reacting molecules
Solubility product constant: the equilibrium constant for a chemical reaction in which a solid ionic compound dissolves to yield its ions in solution.
Hess’ Law: Law which states that the energy change in an overall chemical reaction is equal to the sum of the energy changes in the individual reactions comprising it.