at Capacity of Calorimeter One = 0.03 kJ/.-∆H = (total mass * sp ht * ∆T) + (ht cap * ∆T)= (55 g * 0.004184 kJ/g * -0.2 ) + (0.03 kJ/ * -0.2 )= -0.052 kJ= 0.052 kJ5 g NaCl * 1 mol/58.4 g = 0.086 mol0.052 kJ/0.086 mol = 0.607 kJ/mol∆H = 0.607 kJ/molThe results in Table 2 show that the heat changes are all positive which mean that energy was being added. A reaction that caused a decrease in temperature by removing heat from its surroundings is called endothermic. Precipitation Reactions:For the precipitation reactions, our team chose sodium chloride and silver nitrate for the first reaction and barium chloride and sodium sulfate for the second reaction. The reaction between sodium chloride and silver nitrate formed silver chloride, an insoluble salt. According to Umland and Bellama, All chlorides are soluble [in water] except AgCl and Hg2Cl2 (117). The sodium nitrate would be in solution because all compounds formed of sodium are soluble in water. The reaction between barium chloride and sodium formed barium sulfate, an insoluble salt. According to Umland and Bellama, All sulfates are soluble [in water] except PbSO4, Hg2SO4, SrSO4, and BaSO4 (117). The sodium chloride would be in solution because all compounds formed of sodium are soluble in water. The balanced equations of the two reactions can be seen below. NaCl (aq) + AgNO3 (aq) AgCl (s) + NaNO3 (aq)BaCl (aq) + Na2SO4 (aq) BaSO4 (s) + 2NaCl (aq) The results for the precipitation reactions can be seen in Table 3. For our initial temperature, our team used the temperature of the solution already in the calorimeter before we added the second. Our team always placed either sodium chloride or barium chloride, depending on reaction, in the calorimeter before adding the second compound. Calorimeter Two was used to conduct the experiments. According to Umland and Bellama, Energy changes associated with exothermic changes [have] a negative sign b...
