Question

In problems I, II, and III: Calorimeter constant is 0.00 j/degree C Specific Heat of water or aqueous solutions is 4.18 j/g degree C I. 76.9619 g of metal were heated to 100.7 degree C and poured into a calorimeter containing 46.30 g of water at 25.00 degree C. After stirring, the temperature of the water rose rapidly to 32.40 degree 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 47.00 g of water at 25.05 degree C, 3.0888 g of a salt was added with stirring. As the salt dissolved, the temperature rapidly changed to 31.60 degree C before slowly returning to room temperature. Calculate: c) The Heat of Solution Given that the Heat of Formation of the solid salt is.... -210.01 Kj/mol and the Molecular Mass of the solid salt is 146.30 g/mol Calculate: d) The Heat of Formation of the Solution Kj/mol Given the reaction... AAA + BBB rightarrow CCC You add to a calorimeter 12.0 mL of 4.30 M AAA, 9.0 mL of water, and 11.0 mL of 5.79 M BBB. All of the above solutions were initially at 26.85 degree C. After mixing, the temperature changed to 17.35 degree 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

Answer 1

L 7696 19 g of metal were heated to 100.7 ℃ and poured into a calorimeter containing 46.30 g of water at 25.00 °C. After stirring, the temperature of the water rose rapidly to 32.40 °C before slowly starting to Calculate: a) The Specifie Heat of the metal b) The Atomic Weight Since lost metalQgained,watr we write (mass) (At) (Cp mea)- (mass) (At) (Cp, water 76.9619 g * (100.7-32.40)* Cp, metal46.30 g "(32.40-25.00)*4.18J/g- 76.9619 g * 683 C)*Cp, mea 46.30 g "(7.4 C)*4.18 J g-C 5256.5 g-CCp, meta-1432.15J /g Cp, meta 1432.15 g5256.5 J/g-C Cp metal- 0.272 J/g-C Use the Dulongât Petit law M=3R/sp. ht M-(3) (8.31446 Jmol K)/0272Jg K' M 91.7 g mol Nb niobium