1.) Calculate the energy change for each of the reaction in Parts I- III completed.Remember that heat change for each reaction can be calculated as follows: q=(\text { mass of

solution, } g) \times\left(\text { specific heat, } 4.18 \mathrm{~J} / \mathbf{g}^{\circ} \mathrm{C}\right) \times\left(\Delta T,{ }^{\circ} C\right) a.) mass-Assume that the density of each solution is 1.0 g/ml and therefore the mass of eachsolution is equal to its volume(ml) plus the mass of any solid added. b.) specific heat-Assume a value of 4.18 J/ g°C for each solution. c.) AT, °C-this value can be determined by using the data recorded in your data tables(Maximum T – Minimum T). d.) Be sure to report each value of q using the correct sign (+ or -) based upon the type of reaction (i.e. endothermic or exothermic). Show the reaction and your work for each calculation: Reaction # 1 q1 =___________J Reaction # 2q2 ________=J Reaction # 3q3_________ =J