Calculate the heat capacity of the calorimeter for which the sample data in Figure 2 was collected. Assume that mh=mc=50.0g. 2-3Figure 2: Example GraphTemperature vs. Time: Cold Water + Hot WaterTh = 48.4 °C at time of mixingT = 35.7 °C at time of mixing'T. = 23.8 °C at time of mixing1.234678.10111213Time (min)Once the heat capacity of the calorimeter is known, AH may be calculated for reactions 1, 2 and 3 bymeasuring their temperature increases upon reaction. Since the reactions are done at constant pressure, theheat released by the reaction, q,, is equal to the enthalpy change for that reaction:9r = CATheat released by the system (reaction) = heat absorbed by the surroundings (solution + calorimeter)= Asoln + 9cal = msoln Csoln AT + Ccal ATor9r =-(msoln Csoln + Ccal)ATAT for these reactions is obtained from graphs by extrapolating Tf and T¡ to the time of mixing. The graphswill be similar to Figure 2 except that reactions 2 and 3 will have only two lines (two temperatures) ratherthan three.AH, will be determined for each of reactions 1, 2, and 3. AH3 will also be calculated using Hess's Law asdescribed on the first page of this experiment. Comparison of the experimental and Hess's Law values of AH3will provide a test for Hess's Law.Tem perature ("C)

Given mh = Mass of Hot water = 50.0 gmc = Mass of Cold water = 50.0 gTemperature of Hot water = Th = 48.4 °CTemperature of Cold water = Tc = 23.8 °CResultant tempearture = T = 35.7 °C Specific Heat capacity of water = Cw= 4.184 J/g°CHeat capacity of calorimeter = CHeat absorbed by cold water + heat absorbet by calorimeter = heat released by hot water mc * Cw * (T - Tc)+ C(T - Tc) =- mh * Cw * ( T - Th )50 g * 4.184 J/g°C* (35.7 - 23.8)°C+ C(35.7 - 23.8)°C =- 50 g * 4.184 J/g°C* ( 35.7 - 48.4)°C2489.48 + 11.9C =2656.84C = 14.06 J/°C