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Unit 1 TESTS will be the first week in October. Review materials are available HERE already. Start studying!
Unit Overview
We have already learned how matter is conserved in a chemical reaction, and that a balanced chemical reaction shows that with coefficients that ensure the number of atoms on both sides of the reaction are the same. In this unit we will extend this concept of conservation by also including energy in process.
As chemical bonds break and form, energy stored in those bonds is either released or absorbed. In most cases the amount of energy needed to bond the reactants together is not the same amount of energy needed to bond the products together. That surplus or deficit of energy during the reaction has to be accounted for according to the Law of Conservation of Energy. Excess or needed energy has to be accounted for, and can be absorbed or released in the form of heat, light, or other energy types. This energy can be described in part using the concept of enthalpy.
In this unit we will learn how to track energy changes during a chemical reaction, known as enthalpy. Will will add this information to how we notate chemical reactions, and can use this new data in calculations that we are already familiar with such as stoichiometry.
Later in the unit we will learn how to measure and calculate values for enthalpy including calorimetry, bond enthalpies, and Hess's Law. These are methods used to either measure or estimate values for ΔH, and is where all the data we use in this unit originally came from.
Unit Contents
Section 6: Entropy, Free Energy, and Reaction Spontaneity
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