Endothermic process: Difference between revisions

Latest revision as of 05:29, 16 February 2025

Overview[edit]

An endothermic process is a type of thermodynamic process in which a system absorbs energy from its surroundings in the form of heat. This is in contrast to an exothermic process, where energy is released into the surroundings. Endothermic processes are characterized by a positive change in enthalpy (_H > 0), indicating that the system gains energy.

Mechanism[edit]

In an endothermic process, the energy required to break the bonds of the reactants is greater than the energy released when new bonds are formed in the products. This results in a net absorption of energy. The absorbed energy is typically in the form of heat, which is taken from the surroundings, causing a decrease in the temperature of the environment.

Examples[edit]

Several common processes are endothermic:

Photosynthesis: Plants absorb sunlight to convert carbon dioxide and water into glucose and oxygen.
Melting of ice: Ice absorbs heat from the surroundings to change from solid to liquid.
Evaporation: Liquid water absorbs heat to become water vapor.

Applications[edit]

Endothermic processes have various applications in industry and technology. For example, endothermic reactions are used in cold packs to provide localized cooling. In chemical engineering, endothermic reactions are utilized in processes such as steam reforming to produce hydrogen.

Video[edit]

{{#ev:commons|22.____________________.ogv|thumb|right|An example of an endothermic reaction.}}

Related pages[edit]

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-'''Endothermic process''' refers to a [[chemical reaction]] or physical change in which energy is absorbed from the surroundings, typically in the form of heat. This concept is fundamental in the fields of [[chemistry]], [[physics]], and [[thermodynamics]], playing a crucial role in understanding how substances interact and change. Endothermic processes are characterized by a positive heat flow (into the system) and an increase in [[enthalpy]] ([[ΔH]] > 0). These processes are contrasted with [[exothermic process]]es, where energy is released into the surroundings.
+{{DISPLAYTITLE:Endothermic Process}}
-==Overview==
+== Overview ==
-In an endothermic process, the system absorbs energy from its environment. This energy is usually in the form of thermal energy, but it can also involve other forms of energy, such as electrical energy in the case of electrolysis. The absorbed energy is typically used to break chemical bonds in the reactants, leading to the formation of products. For a process to be considered endothermic, the energy absorbed from the surroundings must exceed the energy released by the formation of new bonds in the product molecules.
+An '''endothermic process''' is a type of [[thermodynamic process]] in which a system absorbs [[energy]] from its surroundings in the form of [[heat]]. This is in contrast to an [[exothermic process]], where energy is released into the surroundings. Endothermic processes are characterized by a positive change in [[enthalpy]] (_H > 0), indicating that the system gains energy.
-==Examples==
+== Mechanism ==
-Common examples of endothermic processes include:
+In an endothermic process, the energy required to break the bonds of the reactants is greater than the energy released when new bonds are formed in the products. This results in a net absorption of energy. The absorbed energy is typically in the form of heat, which is taken from the surroundings, causing a decrease in the temperature of the environment.
-* The melting of ice into water, where heat is absorbed to break the hydrogen bonds between water molecules in the solid state.
-* Photosynthesis, where plants absorb sunlight to convert carbon dioxide and water into glucose and oxygen.
-* The evaporation of water, where heat is absorbed to overcome the forces of attraction between water molecules, allowing them to transition from the liquid to the gaseous state.
-* The cooking of an egg, where heat is absorbed to denature the proteins in the egg white and yolk, changing its structure and state.
-==Thermodynamics==
+== Examples ==
-From a thermodynamic perspective, the key principle governing endothermic processes is the First Law of Thermodynamics, which states that the energy of the universe is constant. Energy can neither be created nor destroyed, only transferred or transformed. In an endothermic reaction, the energy absorbed from the surroundings increases the internal energy of the system, as reflected by a positive change in enthalpy (ΔH > 0).
+Several common processes are endothermic:
-==Significance==
+* [[Photosynthesis]]: Plants absorb sunlight to convert carbon dioxide and water into glucose and oxygen.
-Endothermic processes have significant implications in various scientific and industrial fields. They play a crucial role in weather phenomena, environmental science, and the design of cooling systems. Understanding these processes is also essential in the development of energy storage technologies, such as those used in thermal batteries and endothermic chemical reactions for heat absorption.
+* [[Melting]] of ice: Ice absorbs heat from the surroundings to change from solid to liquid.
+* [[Evaporation]]: Liquid water absorbs heat to become water vapor.
-==See Also==
+== Applications ==
+Endothermic processes have various applications in [[industry]] and [[technology]]. For example, endothermic reactions are used in [[cold packs]] to provide localized cooling. In [[chemical engineering]], endothermic reactions are utilized in processes such as [[steam reforming]] to produce [[hydrogen]].
+== Video ==
+{{#ev:commons|22.____________________.ogv|thumb|right|An example of an endothermic reaction.}}
+== Related pages ==
 * [[Exothermic process]]
 * [[Thermodynamics]]
 * [[Chemical reaction]]
-* [[Enthalpy]]
+* [[Energy transfer]]
-[[Category:Physical chemistry]]
 [[Category:Thermodynamics]]
+[[Category:Chemical processes]]
-{{Chemistry-stub}}