Enthalpy Lab - 1 Josephine Do Uyen Huynh Enthalpy of...

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Unformatted text preview: 1 Josephine Do 2/17/11 Uyen Huynh Enthalpy of Chemical Reactions- Hess’s law The objective of this experiment is to use Hess’s law to determine the enthalpy change of the reaction between aqueous ammonia and aqueous hydrochloric acid and determine the enthalpy of formation of magnesium oxide by calorimetry. The temperature change of the two reactions will be measured, and Hess’ law will be used to determine the enthalpy change, H of a third reaction. Through Δ this experiment, students should be expected to get a better understanding thermodynamics with a calorimeter, how to make a solution of correct concentration, how to accurately time reactions and extract consistent temperatures of valued data, and use percent error to identify how close the obtained data was from accepted value. In reaction three of part 1, the change in enthalpy was determined by multiplying 100 ml of each solution by the density (1.03 g/mL) by the specific heat (4.184 J/g°C) by the change in temperature (T f – T i ). By Hess’s law, we end up with H=3.7 kJ by adding the values of 4.3 kJ and (-.65 kJ, which is a Δ negative value because of the switching of the products with reactants to end up with the proper chemical...
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This note was uploaded on 03/19/2011 for the course CH 204 taught by Professor Leytner during the Spring '08 term at University of Texas.

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Enthalpy Lab - 1 Josephine Do Uyen Huynh Enthalpy of...

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