to the admin. pls. don't delete this i figure it be easier to understand this if it's set up this way because its a prelab.thanks I. 89.7716 g of metal were heated to 99.8 °C and poured into a calorimeter containing 46.20 g of water at 28.45 °C. After stirring, the temperature of the water rose rapidly to 36.25 °C before slowly starting to fall. Calculate: a) The Specific Heat of the metal _____________ b) The Atomic Weight _____________ Calculated using the rule of Dulong and Petit II. To a calorimeter containing 48.80 g of water at 28.85 °C, 7.0545 g of a salt was added with stirring. As the salt dissolved, the temperature rapidly changed to 31.45 °C before slowly returning to room temperature. Calculate: c) The Heat of Solution ______________ Given that the Heat of Formation of the solid salt is.... -180.59 Kj/mol and the Molecular Mass of the solid salt is.......... 143.69 g/mol Calculate: d) The Heat of Formation of the Solution ______________ Kj/mol III. Given the reaction... AAA + BBB ---> CCC You add to a calorimeter 8.0 mL of 5.65 M AAA, 5.0 mL of water, and 12.0 mL of 5.51 M BBB. All of the above solutions were initially at 29.10 °C. After mixing, the temperature changed to 30.60 °C. Assume the density of all solutions is 1.000 g/mL and all solutions have the same specific heat as pure water. Calculate: e) The Heat of Reaction in Kj/mol ______________ i don't know how to get B D and E for A i got .264 for B i divided .264 from 6 but the answer is wrong. i tried it with 6.2 but it i'm still not getting the right answer C=-75.180 D. i really don't have a clue E. i'm given this formula but i'm stuck on limiting reagant (Volume in mL)(Molarity) = millimoles VolumeHCl + VolumeNaOH+ Volumewater = Volumeliquids Temperaturefinal-Temperatureinitial = Temp. Changeliquids (Massliquids)(-Temp. Changeliquids)(4.18 j/gºC) = Energy Change Energy Change/[(1000 j/Kj)(Moles of Limiting Reagent)] = DH Reaction thanks!!!