Question

Review | Constants Periodic Table Part A Calorimetry is a method used to measure changes in enthalpy, or heat, that occur during chemical processes. Two common calorimeters are constant-pressure calorimeters and constant volume or "bomb") calorimeters. Bomb calorimeters are used to measure combustion and other gas- producing reactions, in which the reaction is observed in a strong, sealed vessel. A simple constant-pressure calorimeter can be made from a foam coffee cup and a thermometer, in which energy changes in a reaction are observed via the change in temperature of the solution in the cup. The idea behind calorimeters is that, if they are sufficiently insulated from the outside environment, any energy gained or lost in the chemical reaction will be directly observable as a temperature and/or pressure change in the calorimeter. In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 6.10 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution, AH on of CaCl, is - 82.8 kJ/mol. The specific heat of water is Cs = 4.184 J/(g-K) Express your answer numerically in degrees Celsius. ► View Available Hint(s) PO AED A 0 ? Submit

Answer 1

6-10 gm cache molar mass of cach = 111 g mol > moles of cacla = 6-10 = booss mol Alsoda (CaCl 2) = -87-8 Kolmal a heat released on dissolving ca&z= 82.8 x 0-055 = uss ka - heat released = usso doule loome water, density of water = 1 gmime a mass of water = look I = 100 gm C 6.10 gm Cache a mess of solution= lrot 6.102 106 10 gm Cwater a coolution's 4. love her a heat =mcot 4550= 106-10X40184 XOT 7 Temperatore charge (PT) = 10.3°C Tinisial = 23-0°C a Tfinal = 23+ 10.3 = 33-3 clanswer CScanned with CamScanner