PPT-Enthalpy, entropy, and free energy

604 What does Spontaneous Mean in Chemistry A spontaneous change is a change in a system that proceeds without a net input of energy from an outside source Needs some activation energy to get started. Thermodynamics:. “The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Basic concepts in Big Idea #5. Law of conservation of energy. The Structure . and Dynamics . of Solids. Thomas Hase. Room MAS4.02. E-mail: T.P.A.Hase@warwick.ac.uk. My Research. X-ray (and neutron) scattering from thin films and multilayers. ….. Not much diffraction!. Entropy (S), . Ethalpy. (H) and Gibbs Free Energy (G). What do we know about chemical reactions?. We can write chemical reactions and show how atoms and molecules come together to form products. . We can determine the energy change in a chemical reaction . 12.1 Types of Enthalpy Change . 12.2 Born-Haber Cycles. 12.3 Enthalpy Changes – Enthalpy of Solution. 12.4 Mean Bond Enthalpy. 12.5 Entropy. 12.1 Enthalpy Change – Ionic Compounds. Learning Objectives:. Lecture 4 . The Third Law. “. If the entropy of each element in some crystalline state may be taken as zero at the absolute zero of temperature, every substance has a finite positive entropy, but at absolute zero, the entropy may become zero, and does so become in the case of perfectly crystalline substances. Thermodynamics:. “The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Basic concepts in Big Idea #5. Law of conservation of energy. Chapter 17. Homework. Due with next test. Page 807 . 23-71 . odd. Equations Sheet. Thermodynamics vs. Kinetics. Kinetics deals with . r. ate . of a . reaction, . this depends . on the pathway from reactants to products.. Spontaneous Reaction. A reaction that occurs without outside intervention.. Once it occurs it can be fast or slow.. It can go to completion. (Recall the three products produced :. Precipitate (table F), gas, or water.). Thermodynamic Control of Reactions. Enthalpy. Bond Energies. Forming stronger. bonds favors. reactions.. Molecules with. strong bonds are. more stable.. Entropy. Randomness. Reactions that. Lecture 4 . The Third Law. “. If the entropy of each element in some crystalline state may be taken as zero at the absolute zero of temperature, every substance has a finite positive entropy, but at absolute zero, the entropy may become zero, and does so become in the case of perfectly crystalline substances. Champion Deivanayagam. Center for Biophysical Sciences and Engineering. University of Alabama at Birmingham.. Outline:. Laws of thermodynamics. Enthalpy. Entropy. Gibbs free energy. some examples. Why do chemical reactions happen?. Topic . 15: Energetics (. 8. . hours). 15.1 . Standard enthalpy changes of reaction. 15.1.1 . Define and apply the terms standard state, standard enthalpy change of formation (¬H ) f. . Metabolism. Metabolism. : the sum total of all the chemical reaction that take place to build up and break down the materials needed in an organism. Catabolism. : the breaking down of complex molecules. Define. . temperature. and state the units in which it . is measured.. Define. . heat. and state its units.. Perform. specific-heat calculations.. Solve. . problems involving enthalpies of reaction, enthalpies of formation, and enthalpies of combustion..