Chapter 7: Energy Changes in Chemical Reactions
Chemical reactions involve significant energy changes, either releasing or absorbing energy. Exothermic reactions release heat, often observable through temperature increases or production of light, while endothermic reactions absorb heat, resulting in cooler surroundings. Understanding these energy changes, activation energies, and the role of catalysts is crucial for controlling and optimizing chemical processes in various applications.
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What we have learnt
- Chemical reactions involve breaking and forming bonds, resulting in energy changes.
- Exothermic reactions release energy, typically in the form of heat, while endothermic reactions absorb energy.
- Catalysts increase reaction rates by lowering activation energy without altering the overall energy change.
Key Concepts
- -- Exothermic Reaction
- A reaction that releases energy into its surroundings, causing an increase in temperature.
- -- Endothermic Reaction
- A reaction that absorbs energy from its surroundings, leading to a decrease in temperature.
- -- Activation Energy
- The minimum amount of energy required for reactants to collide effectively and initiate a chemical reaction.
- -- Catalyst
- A substance that increases the rate of a chemical reaction by lowering the activation energy without being consumed.
- -- Energy Profile Diagram
- A graphical representation that shows the energy changes throughout a chemical reaction, illustrating energy of reactants, products, and activation energy.
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