PPT-Calorimetry

Mr Dvorsky SCH 4U1 A calorimeter is an object used for measuring the heat of a chemical reaction or physical change Can be as simple as a pair of cups and a thermometer or as complex as a device attached to the Large Hadron Collider. Introduction Differential scanning calorimetry DSC monitors heat effects associated with phase transitions and chemical reactions as a function of temperature In a DSC the difference in heat flow to the sample and a reference at the same temperature Outline. Types of water. Differential Scanning Calorimetry . Nuclear Magnetic Resonance Spectroscopy . Analytical determination of types of water. Summary. Purpose. Types of water are removed in different ways. Burning of a Match. Zumdahl, Zumdahl, DeCoste, . World of Chemistry. . . 2002, page 293. Energy released to the surrounding as heat. Surroundings. System. (Reactants). D. (PE). Potential energy. (Products). It operates under the law of conservation of energy (what is that?). Heat loss = Heat gained. A device used to measure the absorption or release of this heat is called . Calorimeter. Watch a video lecture for an example.. Quick Review of Concepts. We have been introduced to heat producing (. exothermic. ) reactions and heat using (. endothermic. ) reactions. Heat is a measure of the transfer of . energy. from a system to the surroundings and from the surroundings to a system. Fall, 2010 Indirect Calorimetry 1 Indirect Calorimetry Indirect Calorimetry CALORIMETRY The science that quantifies the heat release from metabolism is termed calorimetry . Figure 4.5 CALORIMETRY D Ohio University (Athens, OH, USA). Uniplast Ltd Co. (Vladimir, . Russia. ). PHENIX Calorimetery Workshop. 12/14/2010 BNL. Main Idea. We have done some preliminary calculations/considerations for the basic parameters of a few more “conventional” options: . Physics 12 . Objectives. Define . specific heat capacity.. Solve problems involving specific heat capacities.. Explain the difference between solid, liquid, and gaseous phases.. Explain in terms of molecular behavior why temperature does not change during a phase change.. calorimetry Enthalpy changes in reactions Calorimetry and heat measurement Hess’s Law Heats of formation Learning objectives • Describe the standard state for thermodynamic functions &# 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. Jukka. . Pekola. , . Low. . Temperature. . Laboratory. Aalto . University. , Helsinki, . Finland. Calorimetry for . measuring the photons. Requirements for calorimetry on single microwave quantum level. Photons from relaxation of a superconducting qubit.. A Calorimeter. A device used to measure the heat involved in a chemical reaction.. The reaction is run in the inner container and the change in the temperature change of the water is measured. The specific heat of the water is KNOWN and the mass of the substance is measured BEFORE the reaction.. Calorimetry Burning of a Match Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 293 Energy released to the surrounding as heat Surroundings System (Reactants) D (PE) Potential energy (Products) 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..