Lecture 30 – Reaction Kinetics and Equilibrium

A set of vocabulary flashcards focused on key terms and concepts in reaction kinetics and equilibrium from Lecture 30.

Catalyst

A substance that increases the rate of a chemical reaction without undergoing any permanent chemical change.

Chemical Equilibrium

A state in which the rates of forward and reverse reactions are the same.

Reversible Reaction

A reaction that can go in either direction, from products to reactants or vice versa.

Equilibrium Constant (K)

A value that indicates the position of a reaction at equilibrium, defined as the concentration of products divided by the concentration of reactants.

Effect of Temperature on Reaction Rate

Raising the temperature increases the energy of reactants, leading to more frequent and forceful collisions, which can double the reaction rate for every 10 °C rise.

Effect of Concentration on Reaction Rate

Increasing concentration enhances the frequency of collisions between reactant molecules, which generally increases the reaction rate.

Forward Reaction

The reaction of a reversible process that proceeds from reactants to products.

Reverse Reaction

The reaction of a reversible process that proceeds from products back to reactants.

Writing an Equilibrium Equation

An equation that shows the relationship between the concentrations of reactants and products at equilibrium, typically represented as K = [products]^[coefficients] / [reactants]^[coefficients].