PPT-5.2 Calorimetry and Enthalpy

Heat Capacity Specific Heat Capacity c the quantity of thermal energy required to raise the temperature of 1 g of a substance by 1C Units are in JgC Heat Capacity Specific heat capacity values can be looked up in tables. 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 6.03 Honors. 6.03 Calorimetry honors. In this experiment, you will determine the quantity of heat involved in two different chemical processes. The heat given off or absorbed will be measured using an insulated calorimeter. Be sure to record all measurements carefully, as you will use the data to calculate the enthalpy change of each process.. 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.. 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 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. 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.. calorimetry Enthalpy changes in reactions Calorimetry and heat measurement Hess’s Law Heats of formation Learning objectives • Describe the standard state for thermodynamic functions &# SiD. ?. Adam Para. ALCPG meeting, December 20, 2007. Other Possible Titles. Homogeneous Dual Readout Calorimeter. A List of Miracles and Why You would Like Them to Happen. Prospects for Crystal-based Hadron Calorimetry. 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.. Reaction Energies. In our earlier discussions of calorimetry, we used . physical. sources of heat (hot metal slug). It is also possible to use . chemical. sources of heat (like hot packs and cold packs).. 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.. 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.