e then done using the salts BaCl2 and NaCl in solid form. Then calculations 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/mol 0.9 kJ/mol
             NaCl 0.6 kJ/mol 1.2 kJ/mol 0.9 kJ/mol
             Table 3: Caliometer 2 - Change in Heat for Precipitation Reactions
             ∆H in Trial 1 ∆H in Trial 2 ∆H in Trial 3
             NaCl & AgNO3 -4.4 kJ/mol -2.8 kJ/mol -2.9 kJ/mol
             BaCl2 & Na2SO4 1.4 kJ/mol -1.3 kJ/mol -1.6 kJ/mol
             Table 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/mol
             Table 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/mol
             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 ...