The first law states that energy cannot be created or destroyed; it can only change forms or be transferred from one part of the system to another.
In an endothermic reaction, the energy required to break the bonds in the reactants is greater than the energy released when new bonds are formed in the products. As a result, the reaction absorbs heat from its surroundings to proceed.
During an adiabatic process, there is no heat transfer into or out of the system. This means that the system is isolated from its surroundings regarding the transfer of thermal energy.
The term 'heat capacity' refers to the amount of heat energy required to raise the temperature of a substance by a given amount. It is a measure of the substance's ability to store thermal energy.
In thermodynamics, a state function (also known as a state property or state variable) is a property that depends only on the current state of a system and is independent of the path or the history by which the system reached that state.
The standard state is defined for each substance, and it includes a particular temperature, pressure, and concentration (usually for solutions) that is considered as the reference or baseline.
The main focus of thermodynamics is the study of energy and its transformations. It deals with understanding how energy is transferred between systems and their surroundings and how it affects the properties and behavior of matter.
Considering entropy is important when predicting the spontaneity of a reaction because entropy represents the dispersal of energy and particles in a system.
The change in enthalpy, often denoted as ΔH, represents the heat transferred during a process that occurs at constant pressure.
When a scientist measures the temperature increase in a solution over time while heating it, they are essentially measuring the average kinetic energy of the molecules in the solution.
The sign of the change in entropy (ΔS) indicates whether a reaction produces more disorder (positive ΔS) or more order (negative ΔS).
Entropy helps to explain why certain processes occur spontaneously and why some natural processes tend to move towards more disordered states.
Gibbs free energy, also known as Gibbs energy or G, represents the energy available in a system to do useful work at constant temperature and pressure.
The decrease in Gibbs free energy during a spontaneous exothermic reaction implies that the reaction is energetically favorable, and the products are more stable than the reactants.
Enthalpy is represented by the symbol "H" and is often used in thermodynamics to describe and analyze energy changes during processes, particularly in systems under constant pressure conditions.
The factor that primarily affects the spontaneity of a reaction is the change in Gibbs free energy
