ations using the data from the experiment were completed enabling us to determine the results found in Table 2. Table 2: Caliometer 1 - Change in Heat for Salts in Water ∆H in Trial 1∆H in Trial 2∆H in Trial 3 BaCl2 0.9 kJ/mol 1.2 kJ/mol0.9 kJ/mol NaCl 0.6 kJ/mol 1.2 kJ/mol0.9 kJ/molTable 3: Caliometer 2 - Change in Heat for Precipitation Reactions ∆H in Trial 1 ∆H in Trial 2∆H in Trial 3NaCl & AgNO3 -4.4 kJ/mol -2.8 kJ/mol-2.9 kJ/molBaCl2 & Na2SO4 1.4 kJ/mol -1.3 kJ/mol-1.6 kJ/molTable 4: Calorimeter 2 - Change in Heat for Strong Acid & Base Reactions Strong Acid & Base ∆H (1M) HCl & (1M) NaOH -85.0 kJ/mol (3M) HCl & (3M) NaOH -63.3 kJ/mol (6M) HCl & (6M) NaOH -79.3 kJ/molTable 5: Calorimeter 1 - Change in Heat for Weak Acid & Base Reactions Weak Acid & Base ∆H (1M) CH3COOH & (1M) NH4OH -48.4 kJ/mol(3M) CH3COOH & (3M) NH4OH -50.7 kJ/mol(6M) CH3COOH & (6M) NH4OH -54.3 kJ/molConstruction of Calorimeters:Two calorimeters were constructed using two Styrofoam cups, one placed inside the other lined with aluminum, and a square cardboard lid. An ideal calorimeter was a good insulator and would have a low heat capacity; the perfect heat capacity would be zero. To measure the heat capacity hot and cold water tests were done and recorded for the calculations for the heat capacities, which are needed for later tests. In order to perform the calculations in all of the experiments the team used the density and specific heat of water, which would cause error in our results. The results were shown in Table 1 and a sample calculation is shown below. Sample Calculation for Calculating Heat Capacity of a Calorimeter:Heat Of Hot H20 (lost) = Hea...
