In general, compounds that release heat when they are formed from their elements have a negative enthalpy, and substances that require heat for their formation have a positive enthalpy. Notice that the enthalpies can be either positive or negative. The reaction isĪnd the enthalpies of the three compounds are given in Table 1. Use the decomposition of ammonium nitrate as an example of an enthalpy calculation. You can consider enthalpy to be chemical energy that is commonly manifested as heat. The equation states that the change in enthalpy during a reaction equals the enthalpy of the products minus the enthalpy of the reactants. Chemists use the term enthalpy for the heat content of a substance or the heat of a reaction, so the H in the previous equation means enthalpy. Throughout this book, the Greek letter delta Δ will be used to symbolize change. Online Quizzes for CliffsNotes Chemistry QuickReview, 2nd Edition.Quiz: Introduction to Oxidation-Reduction Reactions.Introduction to Oxidation-Reduction Reactions. ![]() ![]() Quiz: Heat Capacities and Transformations.Quiz: Introduction to Organic Compounds.Quiz: Compounds with Additional Elements.
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