CHEM 1001 1st Edition Lecture 10Outline of Last Lecture NAOutline of Current Lecture I. The Nature of Energy II. The 1st Law of ThermodynamicsIII. EnthalpyIV. Enthalpies of ReactionCurrent LectureI. The Nature of Energy A. Definitions1. Energy- the capacity to do work or transfer or transfer heat2. Work (w)- energy transferred when an object is moved by a force i. W= F x d [F=force, d= distance]a. F= mass x acceleration (9.8)3. Heat or thermal energy (q)- energy transferred between objects asa result of different temperatures4. Thermodynamics- the study of energy and its transformations These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.5. Thermochemistry- the study of chemical reactions and energy changes involving heatB. Fundamental Forms of Energy 1. Kinetic- due to the motion of an object E = 1/2mv2 = J2. Potential- due to the position or condition of an objecti. Potential energy is energy an object possesses by virtue of its position of chemical composition ii. E = Q1Q2/d 3. Units of energyi. calorie, 1 cal = 4.184 Jii. Calorie, 1kcal = 1000 cal II. The 1st Law of ThermodynamicsA. Total energy of the universe is constant; if the system loses energy, it must be gained by the surroundings and vice versa B. Transfer of internal Energy (E) between a system and its surroundings1. ∆E = Efinal or products – Einitial or reactants C. Relating ∆E to heat and work1. ∆E = q + wi. For q: + means system gains heat, - means system loses heatii. For w: + means work done on system, - means work done by systemiii. For ∆E: + means net gain of energy by system, - means net loss of energy by system D. Endothermic- when heat is absorbed E. Exothermic- when heat is released F. State Functions- a property of a system that depends only on its current state and not on the manner in which the state was achieved 1. Temperature, volume, pressure, internal energy G. Units of P∆V1. Force = Newton (1 N)2. Pressure = Pascal (1 Pa)III. EnthalpyA. Enthalpy, H= heat in processes occurring at constant pressure when the only work is PV work 1. H is a state function that can’t be measured directly i. H = E + PVii. Extensive property (depends on amount)IV. Enthalpies of ReactionA. ∆H = Hfinal or products – Hinitial or reactants B. Endothermic – heat required (from surroundings to system)1. 2KClO3 (s) + heat -> 2KCl (s) + 3 O2 (g)C. Exothermic – heat released (from system to surroundings)1. CH4 (g) + 2 O2 (g) -> Cos (g) + 2H2O (g) +