Chem 222 notes Week 10
Chem 222 notes Week 10 Chem 222
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This 1 page Class Notes was uploaded by Leslie Pike on Friday April 8, 2016. The Class Notes belongs to Chem 222 at Western Kentucky University taught by Darwin Dahl in Spring 2016. Since its upload, it has received 14 views. For similar materials see College Chemistry 2 in Chemistry at Western Kentucky University.
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Date Created: 04/08/16
A reaction is spontaneous if it happens of its own accord, without requiring any outside work. Iron rusting is a spontaneous reaction. Sugar dissolving in water is spontaneous. Spontaneous reactions can be exothermic or endothermic. All spontaneous reactions have an increase in entropy. Entropy is the measure of the disorder of a system. When order increases, entropy decreases. When disorder increases, entropy increases. Think of it this way: All systems tend to maximize entropy, and it takes work to keep them ordered. For instance, if you quit cleaning your room, it would get disordered in a hurry, because disorder is spontaneous. It takes work to keep your room orderly, because your room (like everything else) wants to be as disorganized as possible, and gets disordered of its own accord without any help. Entropy is often symbolized by the capital letter S. Do not confuse with the symbol for sulfur. The change in entropy is calculated as the final entropy minus the initial entropy. Do not confuse entropy with enthalpy. Enthalpy is the internal energy (or internal heat) of a system. Remember than enthalpy is heat, which you can measure with a thermometer.
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