Calorimetry and Enthalpy report - Calorimetry and Enthalpy...

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Calorimetry and EnthalpyHoa ChungChemistry 1A Spring2016, April 12, 2016Objective/PurposeThis experiment has three primary objectives: Find the heat capacity (Cp) of a calorimeter and contents (calibration). Determine the ΔH2, ΔH3the enthalpy of reaction, in kJ/mol Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g) + heat ΔH2MgO(s) + 2H+(aq) → Mg2+(aq) + H2O(l) + heat ΔH3Calculate the ΔH4, the enthalpy of formation, of MgO using Hess’ Law (in kJ/mol). We will assume that the energy exchanged between the calorimeter and the surroundings during andfollowing the reactions is small and at a slow, constant rate. TheoreticalCalorimetry measures the energy that a reaction produces or consumes.Enthalpy, represented by the symbol H, is a property chemists use to describe the heat flowinto or out of a system in a constant-pressure process.The enthalpy of a reaction, ΔHrxn, is defined as the difference between the enthalpies of theproducts and the enthalpies of the reactants. In other words, it is the change in energy for a givenamount of a given reaction.The enthalpy of formation, ΔHf is defined as the enthalpy or heat change that results whenone mole of a compound is formed from its elements. The standard enthalpy of formation defined as the enthalpy of formation measured at 1 atm such that the elements are in their standardstate.
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