PPT-Calorimetry Measuring Heat

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. Measured values show the thermophysical properties of the examined system or sample There are two bas ic types of calorimeters isothermal and adiabatic Constant temperature is sustained in t he isothermal calorimeter t means that the calorimeter is 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). 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 Why do some things get hot more quickly than others?. Temperature. Temperature. . – proportional to the average kinetic energy of the molecules. Energy due to motion. (Related to how fast the molecules are moving). 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.. On the front counter there is a perpetually thirsty bird. Do NOT touch him.. Write down all your . observations. of the motion. Do not try to explain why it’s happening—just look at WHAT is happening. . 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.. : The Experimental Measurement of Heat. Outline. Background. Exothermic . vs. Endothermic Reactions. Heat Capacity. Specific Heat. Specific Heat of Selected Substances and Mixtures. Relevance. Background. cal. /g·°C) to consume the drink?.  . a. Calculate . the energy expended (in . Cal. ) to consume a 12-oz beer (about 355 mL) if the beer is initially at 4.0°C. Assume the drink is mostly water and its density is 1.01 g/. Calorimetry. 1. Temperature and Energy. 2. We relate energy and temperature by discussing a substance’s heat capacity.. Heat Capacity = heat required to raise temp. of an object by 1. o. C. more heat is required to raise the temp. of a large sample of a substance by 1. 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) A student doing an experiment . inserts.  0.190 kg of . an unknown metal, originally at 100.0°C into . a 0.315 kg aluminum calorimeter cup containing 0.100 kg of water at 24°C. The mixture (and the cup) comes . III. A 0.5269 g of octane is placed in a bomb calorimeter known to have a heat capacity of 11.3 kJ/. o. C.. The octane, a component of gasoline, is ignited in the presence of excess oxygen. The temperature is increased by 2.25.