PPT-Enthalpy

Internal Energy Equation ΔE Q W Q PΔV If the reaction is carried out at a constant volume ΔV 0 then ΔE Q If volume is constant any heat added or removed changes the internal energy. is the enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions. . Enthalpy Change of reaction . is the enthalpy change that accompanies a chemical reaction in molar quantities expressed in a chemical equation. . 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). n, For a solution prepared using 1 kg of solvent, water and m ()()HaqwMHaqHaq111 kg m==
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The chemical potential of the solvent in an aqueous solution is related to the molality of solute j, m () n, For a solution prepared using 1 kg of solvent, water and m ()()HaqwMHaqHaq111 kg m==
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The chemical potential of the solvent in an aqueous solution is related to the molality of solute j, m () 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.. 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:. Thermodynamics. is the study of energy and how it is interconverted.. First law of thermodynamics. – energy cannot be created or destroyed; it can only be converted from one form to another (. law of conservation of energy. 2016. School and Workshop . in Cryogenics . and Quantum Engineering. 26. th. September - 3. rd. October 2016. Aalto University, Espoo, Finland. Introduction to Dilution . Refrigerators. . Part I-. Heat Capacity. Specific Heat Capacity (c): . the quantity of thermal energy required to raise the temperature of 1 g of a substance by 1°C.. Units are in J/g∙°C. Heat Capacity. Specific . heat capacity values can be looked up in tables. Lecture 8 Topics. . Brown chapter 5. 8.1. :. . Kinetic . vs. potential energy. . 5.1. 8.2. :. . Transferring . energy as heat & work. Thermal energy. 8.3: . System . vs. surroundings. 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.. 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. 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.. by. Basharat Jamil. Syllabus. Unit–I : Thermodynamic Relations:. . Maxwell relations, . Clausius-Clapeyron. equation, Joule-Thomson coefficient, Relations involving enthalpy, internal energy, entropy, specific heats, volume expansivity, isothermal and adiabatic compressibility, Ideal and real gas behavior, Real gas equations of state, Generalized charts for: compressibility, changes of enthalpy and entropy at constant temperature, Availability and irreversibility..