Understand the law of conservation of energy in relation to chemical reactions, stating that the total amount of energy at the conclusion of a reaction equals the amount before it began.
Explain that in a reaction that transfers energy to the surroundings, the resulting product molecules inherently possess less energy than the initial reactants.
Define an exothermic reaction as a chemical process that transfers thermal energy to the environment, measurable as a temperature increase in the surroundings.
Identify common examples of exothermic reactions such as typical combustion, diverse oxidation reactions, and acid-base neutralization.
Evaluate practical everyday uses of exothermic reactions such as self-heating food cans and commercially available hand warmers.
Define an endothermic reaction as a chemical process that actively absorbs energy from the environment, measurable as a temperature decrease in the surroundings.
Identify common examples of endothermic reactions including thermal decomposition processes and the specific reaction between citric acid and sodium hydrogencarbonate.
Evaluate practical everyday uses of endothermic reactions such as instant sports injury cold packs.
Distinguish reliably between exothermic and endothermic reactions strictly based upon observational measurement of surrounding temperature changes.
Evaluate the utility and viability of various applications of exothermic and endothermic reactions given necessary contextual information.
Execute practical investigations determining the specific variables that influence recorded temperature changes in different reacting solutions.
