PPT-THERMOCHEMISTRY ENERGETICS/ENTHALPY

INTRODUCTION All reactions require energy to break bonds in the reactants and all reactions give off energy when new bonds form to make products The difference in energy required to break the bonds and to make the new bonds can tell you whether the reaction is endothermic or exothermic . Glycolysis. C483 Spring 2013. 1. The . conversion of pyruvate to ethanol also causes the ________. . A) oxidation of NADH . B) production of ADP . C) consumption of O2 . D) generation of an ion gradient across mitochondrial membranes . IB Topics 5 & 15. PART . 1: Heat and . Calorimetry. Above: thermit rxn. Energy: . a measure of the ability to do work.. Work: . to move an object against an opposing force.. Energy (J) = Force (N) x Distance (m). Objectives. Recall the definition of standard enthalpy changes of reaction, formation, combustion. Edexcel AS Chemistry p79. Standard Enthalpies. When we compare enthalpy changes of reactions we use . 2. . Know and be able to account for the trends in reactivity with water. , the relative solubility of the hydroxides and sulfates. . The Trend . Hydroxides increase in solubility down the group.. Sulfates decrease in solubility down the group.. Enthalpy. Enthalpy (H)is the total amount of energy contained within a substance. Included all forms of energy, kinetic, potential…. Very difficult to measure all forms of energy within a substance, therefore a change in enthalpies is measured whenever a change occurs.. calorimetry Enthalpy changes in reactions Calorimetry and heat measurement Hess’s Law Heats of formation Learning objectives • Describe the standard state for thermodynamic functions &# g. recall the stages involved in the formation of a solid ionic crystal from its elements and that this leads to a measured value for the lattice energy (students will not be expected to draw the full Born-Haber cycles). 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.). Enthalpy . is a state function . (the pathway does not matter) with . the symbol . H. ..  . H . = E . P V. E . is the internal energy of the system, P is the pressure of the system, and V is the volume of the system.. Lecture Presentation. © 20. 12. Pearson Education, Inc.. © 2012 Pearson Education, Inc.. Energy. Energy. is the ability to do work or transfer heat.. Energy used to cause an object that has mass to move is called . 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. and that this was an ea specific molecular keyhole like a modern drug Thus for instance we have the irritants or stimulants the anti-irritants or sedatives nd functions of the organism circulation r A form of energy. Flows from warmer objects to cooler objects. Represented by the variable “q”. Measured by units: calorie or joule. 1 J = 0.2390 . cal. 4.184 J = 1 . cal. 1000 . cal. = 1 . kilocalorie . Change. First Law of Thermodynamics. Heat . (q. ). ,. work (. w. ) and internal energy (. E. ). Calculation of heat gained or lost by system. Calorimeter for measuring heat exchange (between system and surrounding;.