Almost all chemical reactions involve a loss or gain of heat. This change in heat is called enthalpy. The goal of this experiment is to calculate enthalpy for three different reactions. To calculate the enthalpy of a reaction, a calorimeter is used to measure the change in heat energy from mixing different substances. The change of temperature is found by comparing the change in temperature of the system to the temperature of the surroundings. For a calorimeter, a Styrofoam cup place in a beaker is used. The Styrofoam of the cup minimizes heat loss and the beaker keeps the cup in a stable position. Hot and cold water were mixed in the calorimeter to calibrate it and determine its heat capacity, which comes into play in the three reactions tested.
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Methods The procedure performed came from pages 106-108 of the lab manual (French et al, 106-108). No changes were made to the procedure.
Discussion
The heat capacity of the calorimeter was determined to be 19.3 J/˚C. For reaction 1, which was between NaOH and HCl, the enthalpy of the reaction was -45.7 kJ/mol. For reaction 2, which was between NaOH and NH_4 Cl, the enthalpy of the reaction was -8.67 kJ/mol. For reaction 3, which was between HCl and NH_3, the enthalpy of the reaction was -46.2 kJ/mol. The enthalpy of reaction 3 determined by Hess’s Law and the results of reactions 1 and 2 was -37 kJ/mol. The percent error for the enthalpy of reaction 3 acquired from the in-lab procedure was 13%. The percent error for the enthalpy of reaction 3 acquired using Hess’s Law was 30%. One significant correlation between all of the enthalpies calculated is that all of them are negative, showing that heat was lost in all of the reactions, making them exothermic. As for the percent errors, there was less error when the data acquired was recorded by observing a performed reaction. Guessing the enthalpy using Hess’s Law and the results of the other reactions introduced more error into the calculation. One source of error could be that when the reactant was being poured into the calorimeter, leaving the lid open for too long let too much heat loose, which would affect the results. This would have affected reactions 1 and 2, and that increased percent error would affect the enthalpy of reaction 3 calculated using Hess’s Law. It affected the enthalpy calculated from the in-lab results less because the was only one reaction where that error could affect the
Methods The procedure performed came from pages 106-108 of the lab manual (French et al, 106-108). No changes were made to the procedure.
Discussion
The heat capacity of the calorimeter was determined to be 19.3 J/˚C. For reaction 1, which was between NaOH and HCl, the enthalpy of the reaction was -45.7 kJ/mol. For reaction 2, which was between NaOH and NH_4 Cl, the enthalpy of the reaction was -8.67 kJ/mol. For reaction 3, which was between HCl and NH_3, the enthalpy of the reaction was -46.2 kJ/mol. The enthalpy of reaction 3 determined by Hess’s Law and the results of reactions 1 and 2 was -37 kJ/mol. The percent error for the enthalpy of reaction 3 acquired from the in-lab procedure was 13%. The percent error for the enthalpy of reaction 3 acquired using Hess’s Law was 30%. One significant correlation between all of the enthalpies calculated is that all of them are negative, showing that heat was lost in all of the reactions, making them exothermic. As for the percent errors, there was less error when the data acquired was recorded by observing a performed reaction. Guessing the enthalpy using Hess’s Law and the results of the other reactions introduced more error into the calculation. One source of error could be that when the reactant was being poured into the calorimeter, leaving the lid open for too long let too much heat loose, which would affect the results. This would have affected reactions 1 and 2, and that increased percent error would affect the enthalpy of reaction 3 calculated using Hess’s Law. It affected the enthalpy calculated from the in-lab results less because the was only one reaction where that error could affect the