L07 Chem 151 Lecture Notes - Lecture 7: Magnesium Oxide, Exothermic Process, Heat Capacity
14 Mar 2016
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Practice exam (blank and key) will be posted this thursday (3/10) by 5 pm. Mentor q&a session on sunday, 3/20, from 7-9pm in ls400. Use calorimetry and apply hess"s law to determine the enthalpy of formation, deltah_f of magnesium oxide. Use calorimetry to measure the amount of heat evolved for a neutralization reaction and determine the concentration of a strong base. Endothermic = deltah > 0, heat is absorbed. Exothermic = deltah < 0, heat is evolved. When a reaction is exothermic, the heat evolved from the reaction will be absorbed by the solvent, raising its temperature. No, deltah cannot be both greater and less than 0. But, an exothermic process can combine with an endothermic process. When the two processes combine, the net amount of heat produced is less than the original exothermic reaction. Hess"s law: the enthalpies of reactions can be added in the same manner as the reaction equations.
