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Unformatted text preview: follows: H rxn, (a) = -59.8 kJ/mol, H rxn, (b) = -53.6 kJ/mol, H rxn, (c) = -57.5 kJ/ mol, and H rxn, (d) = -56.2 kJ/mol. Using these experimentally-derived enthalpy values and setting up a Hess Law problem, a value for the enthalpy of the neutralization for (d) was calculated to be -51.3 kJ/mol, which constituted an 8.7% error from the directly-calculated value. Considering this relatively small error value, it can be concluded that the experiment was conducted well and that the theory behind calorimetry, including the Laws of Thermodynamics, are accurate for this experiment....
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- Fall '07