Entropy is a concept from thermodynamics that refers to the degree of disorder or randomness in a system. In statistical mechanics, it is often defined as the number of microstates (arrangements of particles or energy levels) that correspond to a given macrostate (observable properties like temperature, pressure, or volume). The greater the number of microstates,…
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…
Hess’s law is a fundamental principle in chemistry that states that the total enthalpy change of a chemical reaction is independent of the pathway between the initial and final states. In other words, if a reaction can occur by multiple paths, the change in enthalpy will be the same regardless of the specific path taken.…
Heat capacity is the amount of heat energy required to raise the temperature of a substance by one degree Celsius or one Kelvin. It is a physical property of a substance that measures its ability to store heat energy. Heat capacity is usually denoted by the symbol “C” and has units of joules per degree…
Work and heat are both important concepts in thermodynamics. In thermodynamics, work is defined as the energy transferred when a force is applied over a distance, while heat is defined as the energy transferred between two objects at different temperatures. In terms of pressure and volume, work is calculated as the product of the pressure…
Internal energy refers to the total energy that is contained within a system. This energy includes the kinetic and potential energies of the particles within the system, as well as any other forms of energy that may be present, such as chemical energy, thermal energy, and nuclear energy. The internal energy of a system is…
The first law of thermodynamics, also known as the law of conservation of energy, states that energy cannot be created or destroyed, only transformed from one form to another or transferred from one system to another. In other words, the total amount of energy in a closed system remains constant. This law is fundamental to…
In thermodynamics, a state function is a property of a system that depends only on the current state or condition of the system and not on how the system arrived at that state. State functions are also known as state variables or state quantities. Some common examples of state functions include: State functions are extremely…
In thermodynamics, properties of matter can be classified as either intensive or extensive. Intensive properties are properties that do not depend on the amount of matter present. Examples of intensive properties include temperature, pressure, density, and specific heat capacity. These properties are useful in describing the state of a system and can be used to…
Square planar refers to the geometry or arrangement of atoms or ligands around a central atom in a molecule or ion, where the central atom is located at the center of a square plane. In a square planar arrangement, the central atom is surrounded by four ligands or atoms that are arranged in a flat,…
