Why some reactions release heat while others consume it
In short: Understanding the fundamental difference between exothermic and endothermic reactions requires looking at how energy is stored within chemical bonds. This video explains how to visualize these shifts using reaction profiles.
Chemical reactions are defined by the energy difference between reactants and products. In exothermic reactions, such as combustion or oxidation, products have less energy than the starting materials, meaning heat is released into the surroundings. Conversely, endothermic reactions—like the thermal decomposition of calcium carbonate—require an input of energy, resulting in products with higher energy levels than the reactants.
The video explores how to interpret reaction profile diagrams to map these changes. Activation energy represents a fundamental principle, denoting the lowest level of power needed for colliding particles to undergo a chemical transformation. The presentation demonstrates how to represent this threshold on both types of profiles to determine a reaction's feasibility.
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Sources
- Summary by Intellect · source: GCSE Chemistry - Exothermic & Endothermic Reactions - Reaction Profiles | Activation Energy
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