Chem Notes Week 6
Chem Notes Week 6 CHE 106 - M001
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CHE 106 - M001
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This 3 page Class Notes was uploaded by Andrea Scota on Saturday October 10, 2015. The Class Notes belongs to CHE 106 - M001 at Syracuse University taught by R. Doyle in Fall 2015. Since its upload, it has received 56 views. For similar materials see General Chemistry Lecture I in Chemistry at Syracuse University.
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Date Created: 10/10/15
mentioned in class Chem Notes Week 6 TEXTBOOK CHAPTER 5 Thermochemistry is examining the relationships between chemical reactions and energy changes that involve heat Energy 51 0 Work is the energy used to cause an object to move against a force and heat is the energy used to cause the temperature of an object to increase 0 Can be electromagnetic radiation associated with the random movement of molecules or the energy held in bonds Objects can possess the which depends on its mass and speed we are interested in the kinetic energy of atoms and molecules Objects can possess or by virtue of its position relative to other objects g is gravity h is weight m is mass electrostatic potential energy Eel arises from interactions between charged particles and is proportional to electrical charges on 2 interacting objects q1 and q2 inversely proportional to a distance d separating them Eel KQlQZd k is constant 899 X 109 JmCZ O C coulomb unit of electrical charge j joule unit of energy When 01 and Oz are both positive they repel each other and potential energy decreases when they are both negative they attract each other and the potential energy increases F 39 The unit of energy is a 39 0 Energy change in chemical reactions 0 Systems may be open closed or isolated Open energy and matter can be exchanged with surroundings Closed energy can be exchanged with surroundings but not matter 0000 Isolated neither Magnitude of work is products of force push or pull on object and distance object moves o W fd The First Law of Thermodynamics 52 0 Recall energy can be neither created nor destroyed 0 We are concerned with the change in E 0 AE E nal Einitial can either be positive the system gained energy or negative the system lost energy of a systein in magnitude or work is don t on or by a system 0 Heat added or subtracted q work w 0 AE qw When a takes in heat it is r when a generates heat it is o E has xed values on temperature and pressure 0 Internal energy is a state function a property of a system that is determined by specifying systems conditions or state 0 The value of a state function depends only on the present state of the system not the path the system took to reach the state Enthalpy 53 Enthalpy H is internal energy the product of pressure P and volume V o H EPV Pressure volume work is the work involved in the expansion of compression of gases PV when w PAV when pressure is constant AV V nal Vinitial P is always gt 0 0 Pressure atm multiplied by volume L I L atm 1013J When change occurs in constant pressure AH AEPV qp w W qp The change in enthalpy equals the heat gained of lost at constant pressure Enthalpies of Reaction 54 Enthalpy change for a chemical reaction is AH Hproducts Hreactants called the enthalpy of a reaction the heat of a reaction 0 EX when 2 mol of H2 burns to form 2 mol of H20 g at constant pressure the system releases 4836 kJ 2H2 g 02 g gt 2H20 g AH 4836 kJ negative sign shows its exothermic coefficients show the number of moles of each substance in a balanced chemical equation producing associated enthalpy change thermochemical equations Guidelines for using thermochemical equations and enthalpy diagrams O O 1 Enthalpy is an extensive property The magnitude of AH is proportional to the amount of reactant consumed in the process 2 The enthalpy change for a reaction in magnitude but opposite in sign to AH for the reverse reaction When reverse reaction we reverse the roles of the products and reactants AH of before 3 The enthalpy change for a reaction depends on the states of reactants and products It is important to specify the states of reactants and products
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