Catalysis refers to the process in which a catalyst increases the rate of a chemical reaction by providing an alternative pathway with lower activation energy. There are two types of catalysis: homogeneous catalysis and heterogeneous catalysis. Homogeneous catalysis involves a catalyst that is in the same phase (i.e., gas, liquid, or solid) as the reactants.…
The rate of a chemical reaction is the change in the concentration of reactants or products per unit time. The rate law for a chemical reaction describes how the rate of the reaction depends on the concentrations of the reactants. There are different rate laws for different types of reactions, but two common types are…
A rate law is an equation that describes how the rate of a chemical reaction depends on the concentrations of the reactants. It is also known as the rate equation or the rate expression. The general form of a rate law is: Rate = k [A]^m [B]^n Where: The orders m and n are usually…
In chemistry, the order of a reaction refers to the exponent to which the concentration of a reactant is raised in the rate equation of a reaction. The molecularity of a reaction refers to the number of molecules, ions or atoms that participate in the reaction’s rate-determining step. For example, consider the reaction: A +…
The electrochemical series is a list of metals and non-metals arranged in order of their standard electrode potentials (reduction potentials) or their tendency to undergo reduction. It is also known as the activity series. The electrochemical series is a useful tool in predicting the outcome of redox reactions, especially in electrolytic cells and in electrochemical…
Acids and bases are fundamental concepts in chemistry that are used to describe the properties of various chemical substances. The Bronsted and Lewis concepts are two different approaches used to define acids and bases. The Bronsted-Lowry concept defines an acid as a substance that donates a proton (H+) and a base as a substance that…
The common ion effect is a phenomenon in which the solubility of a slightly soluble salt is decreased by the presence of a common ion in the solution. This effect is due to the principle of Le Chatelier’s principle, which states that a system at equilibrium will shift to counteract any stress placed upon it.…
The criteria for equilibrium and spontaneity are closely related to the concept of Gibbs free energy, which is a thermodynamic function that measures the energy available in a system to do useful work. The Gibbs free energy is defined as follows: ΔG = ΔH – TΔS where ΔG is the change in Gibbs free energy,…
Gibbs energy, also known as Gibbs free energy, is a thermodynamic quantity that measures the amount of energy available to do useful work in a chemical reaction or physical process at constant temperature and pressure. It is denoted by the symbol G and has units of joules (J) or kilojoules (kJ) per mole. Gibbs energy…
The enthalpy of reaction (ΔHrxn) is the amount of heat released or absorbed during a chemical reaction at a constant pressure. It represents the change in the enthalpy of the system as reactants are transformed into products. If the enthalpy of reaction is negative (ΔHrxn < 0), it means that the reaction is exothermic, and…
