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Endothermic vs Exothermic
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Table of Contents
Examples of Endothermic and Exothermic Processes
Demonstrations You Can Perform
Endothermic vs Exothermic Comparison
Resources and Further Reading
By
Anne Marie Helmenstine, Ph.D.
Anne Marie Helmenstine, Ph.D.
Chemistry Expert
- Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
- B.A., Physics and Mathematics, Hastings College
Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels.
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Updated on July 30, 2024
Many chemical reactions must absorb energy to proceed. These are endothermic reactions. Endothermic reactions cannot occur spontaneously. Work must be done to get these reactions to occur. When endothermic reactions absorb energy, a temperature drop is measured during the reaction. Endothermic reactions are characterized by positive heat flow (into the reaction) and an increase in enthalpy (+ΔH).
Other chemical reactions release energy in the form of heat, light, or sound. These are exothermic reactions. Exothermic reactions may occur spontaneously and result in higher randomness or entropy (ΔS > 0) of the system. They are denoted by a negative heat flow (heat is lost to the surroundings) and a decrease in enthalpy (ΔH < 0). In the lab, exothermic reactions produce heat or may even be explosive.
Examples of Endothermic and Exothermic Processes
Photosynthesis is an example of an endothermic chemical reaction. In this process, plants use the energy from the sun to convert carbon dioxide and water into glucose and oxygen. This reaction requires 15MJ of energy (sunlight) for every kilogram of glucose produced:
sunlight + 6CO2(g) + H2O(l) = C6H12O6(aq) + 6O2(g)
Other examples of endothermic processes include:
- Dissolving ammonium chloride in water
- Cracking alkanes
- Nucleosynthesis of elements heavier than nickel in stars
- Evaporating liquid water
- Melting ice
An example of an exothermic reaction is the mixture of sodium and chlorine to yield table salt. This reaction produces 411 kJ of energy for each mole of salt produced:
Na(s) + 0.5Cl2(s) = NaCl(s)
Other examples of exothermic processes include:
- The thermite reaction
- A neutralization reaction (e.g., mixing an acid and a base to form a salt and water)
- Most polymerization reactions
- Combustion of a fuel
- Respiration
- Nuclear fission
- Corrosion of metal (an oxidation reaction)
- Dissolving an acid in water
Demonstrations You Can Perform
Many endothermic and exothermic reactions involve toxic chemicals, extreme heat or cold, or messy disposal methods. An example of an easy endothermic reaction is dissolving potassium chloride (sold as a salt substitute) in your hand with water. An example of a quick exothermic reaction is dissolving powdered laundry detergent in your hand with a bit of water.
These endothermic and exothermic demonstrations are safe and easy:
- Exothermic Reactions to Try: Heat things up with one of these simple exothermic reaction demonstrations.
- Create an Endothermic Reaction: Some endothermic reactions get cold enough to cause frostbite. Here is an example of a reaction safe enough for kids to touch.
- How to Create an Exothermic Chemical Reaction: Some exothermic reactions produce flames and get extremely hot (like the thermite reaction). Here is a safe exothermic reaction that produces heat but will not start fires or cause a burn.
- Make Hot Ice From Vinegar and Baking Soda: You can use sodium acetate or "hot ice" as an endothermic or exothermic reaction, depending on whether you are crystallizing or melting the solid.
Endothermic vs Exothermic Comparison
Here is a quick summary of the differences between endothermic and exothermic reactions:
| Endothermic | Exothermic |
| heat is absorbed (feels cold) | heat is released (feels warm) |
| energy must be added for reaction to occur | reaction occurs spontaneously |
| disorder decreases (ΔS < 0) | entropy increases (ΔS > 0) |
| increase in enthalpy (+ΔH) | decrease in enthalpy (-ΔH) |
Endergonic and Exergonic Reactions
Endothermic and exothermic reactions refer to the absorption or release of heat. Other types of energy may be produced or absorbed by a chemical reaction (examples include light and sound). In general, reactions involving energy may be classified as endergonic or exergonic, An endothermic reaction is an example of an endergonic reaction. An exothermic reaction is an example of an exergonic reaction.
Key Facts
- Endothermic and exothermic reactions are chemical reactions that absorb and release heat, respectively.
- Photosynthesis is a good example of an endothermic reaction. Combustion is an example of an exothermic reaction.
- The categorization of a reaction as endothermic or exothermic depends on the net heat transfer. In any given reaction, heat is both absorbed and released. For example, energy must be input into a combustion reaction to start it (lighting a fire with a match), but then more heat is released than was required.
Resources and Further Reading
- Qian, Y.‐Z., et al. “Diverse Supernova Sources for the r‐Process.” The Astrophysical Journal, vol. 494, no. 1, 10 Feb. 1998, pp. 285-296, doi:10.1086/305198.
- Yin, Xi, et al. “Self-Heating Approach to the Fast Production of Uniform Metal Nanostructures.” Chemistry of Nanomaterials for Energy, Biology and More, vol. 2, no. 1, 26 Aug. 2015, pp. 37-41, doi:10.1002/cnma.201500123.
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Your Citation
Helmenstine, Anne Marie, Ph.D. "Understanding Endothermic and Exothermic Reactions." ThoughtCo, Jul. 31, 2024, thoughtco.com/endothermic-and-exothermic-reactions-602105.Helmenstine, Anne Marie, Ph.D. (2024, July 31). Understanding Endothermic and Exothermic Reactions. Retrieved from https://www.thoughtco.com/endothermic-and-exothermic-reactions-602105Helmenstine, Anne Marie, Ph.D. "Understanding Endothermic and Exothermic Reactions." ThoughtCo. https://www.thoughtco.com/endothermic-and-exothermic-reactions-602105 (accessed September 3, 2024).
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