Energy Changes in Chemical Reactions
This page delves into the fundamental concepts of exothermic reactions and endothermic reactions, their characteristics, and practical applications. It also covers methods for measuring energy transfer and introduces reaction profiles.
Definition: An exothermic reaction is one which transfers energy to the surroundings, resulting in a rise in temperature.
Examples of exothermic reactions include combustion, neutralization reactions, and many oxidation reactions. The document highlights a practical application of exothermic reactions in hand warmers, which utilize the oxidation of iron in air to release energy.
Definition: An endothermic reaction is one which takes in energy from the surroundings, leading to a decrease in temperature.
The page outlines a practical method for measuring energy transfer in chemical reactions, specifically focusing on the reaction between hydrochloric acid and sodium hydroxide. This experiment involves using a polystyrene cup and water bath to minimize energy loss to the surroundings.
Highlight: To prevent energy loss during experiments, insulation techniques such as using a polystyrene cup, cotton wool, and a lid are employed.
The document introduces reaction profiles, which are diagrams showing the relative energies of reactants and products throughout a reaction. These profiles illustrate key concepts such as activation energy and overall energy change.
Vocabulary: Activation energy is the minimum amount of energy that reactants need to collide with one another and initiate a reaction.
The page also covers bond energies, explaining that bond-breaking is an endothermic process, while bond-forming is exothermic. This concept is crucial for understanding why some reactions are overall exothermic or endothermic.
Example: In the reaction between chlorine and bromine with hydrogen, the difference in bond strengths affects the overall energy change of the reaction.
Finally, the document introduces electrochemical cells, explaining their basic components and factors affecting their voltage. It briefly mentions fuel cells and batteries, highlighting the difference between non-rechargeable and rechargeable batteries.
Definition: An electrochemical cell is a basic system made up of two different electrodes in contact with an electrolyte, capable of producing electricity.
This comprehensive overview provides a solid foundation for understanding energy changes in chemical reactions and their practical applications.
