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11-SEPTEMBER-2008 13:54:10 - Calorimetry The world's first ice-calorimeter, used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black's prior discovery of latent heat. These experiments mark the foundation of thermochemistry. The world's first ice-calorimeter, used in the winter of 1782-83, by Antoine Lavoisier and Pierre-Simon Laplace, to determine the heat evolved in various chemical changes; calculations which were based on Joseph Black's prior discovery of latent heat. These experiments mark the foundation of thermochemistry. Calorimetry is the science of measuring the heat of chemical reactions or physical changes. Calorimetry involves the use of a calorimeter. The word calorimetry is derived from the Latin word calor, meaning heat. Scottish physician and scientist Joseph Black, who was the first to recognize the distinction between heat and temperature, is said to be the founder of calorimetry.1 Indirect calorimetry calculates heat that living organisms produce from their production of carbon dioxide and nitrogen waste frequently ammonia in aquatic organisms, or urea in terrestrial ones, OR from their consumption of oxygen. Lavoisier noted in 1780 that heat production can be predicted from oxygen consumption this way, using multiple regression. The Dynamic Energy Budget theory explains why this procedure is correct. Of course, heat generated by living organisms may also be measured by direct calorimetry, in which the entire organism is placed inside the calorimeter for the measurement. Contents 1 Types 1.1 Constant-volume 1.2 Constant-pressure 2 See also 3 References Types Calorimetry is performed using one of two methods: constant volume or constant pressure. Constant-volume Constant-volume calorimetry is calorimetry performed at a constant volume. This involves the use of a constant-volume calorimeter. No work is performed in constant-volume calorimetry, so the heat measured equals the change in internal energy of the system. The equation for constant-volume calorimetry is the heat capacity at constant volume is assumed to be constant: q = C_V \Delta T = \Delta U \, where ΔU is change in internal energy, ΔT is change in temperature and CV is the heat capacity at constant volume. Since in constant-volume calorimetry the pressure is not kept constant, the heat measured does not represent the enthalpy change. Constant-pressure Constant-pressure calorimetry is calorimetry performed at a constant pressure. This involves the use of a constant-pressure calorimeter. The heat measured equals the change in internal energy of the system minus the work performed: q = \Delta U - w \, Since in constant-pressure calorimetry, pressure is kept constant, the heat measured represents the enthalpy change: q = \Delta H = H_\mathrmfinal - H_\mathrminitial \, This formula is a simplified representative of Hess's Law. See also Accelerating rate calorimetry Differential scanning calorimetry Isothermal titration calorimetry Respirometry Thermodynamic databases for pure substances Thermochemistry References ^ Laider, Keith, J. 1993. The World of Physical Chemistry. Oxford University Press. ISBN 0-19-855919-4. v d e Analytical chemistry Instrumentation Atomic absorption spectrometer · Flame emmission spectrometer · Gas chromatograph · High performance liquid chromatograph · Infrared Spectrometer · Mass spectrometer · Melting point apparatus · Microscope · Spectrometer · Spectrophotometer Techniques Calorimetry · Chemometrics · Chromatography · Electrochemistry · Gravimetric analysis Sampling Coning and quartering · Dilution · Dissolution · Filtration · Masking · Pulverization · Sample preparation · Separation process · Sub-sampling Prominent publications Analytical chemistry Chemistry Retrieved from http://en..org/wiki/Calorimetry Categories: Heat | Thermodynamics | Calorimetry Views Article Discussion this page History Personal tools Log in / create account Navigation Main page Contents Featured content Current events Random article Search Go Search Interaction Community portal Recent changes Contact Donate to Help Toolbox What links here Related changes Upload file Special pages Printable version Permanent link Cite this page Languages Bosanski ÄŒesky Dansk Deutsch Español Ù?ارسی Français Italiano Nederlands Polski Português РуÑ?Ñ?кий SlovenÄ?ina УкраїнÑ?ька This page was last modified on 8 August 2008, at 02:4
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