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11 Nov 2019
This question has multiple parts. Work all the parts to get the most points. In a coffee-cup calorimeter, 1.17 g NH_4NO_3 was mixed with 55.00 g water at an initial temperature 25.00 degree c. After dissolution of the salt, the final temperature of the calorimeter contents was 23.34 degree C. Assuming the solution has a heat capacity of 4.18 J/g middot degree C, and assuming no heat loss to the calorimeter, calculate the enthalpy of solution (Delta H_soln) for the dissolution of NH_4NO_3 in units of kJ/mol. Delta H_soln = k.J/mol In a coffee-cup calorimeter, 1.17 g NH_4NO_3 was mixed with 55.00 g water at an initial temperature 25.00 degree C. After dissolution of the salt, the final temperature of the calorimeter contents was 23.34 degree C. If the enthalpy of hydration for NH_4NO_3 is -630. kJ/mol, calculate the lattice energy of NH_4NO_3. Lattice energy = kJ/mol
This question has multiple parts. Work all the parts to get the most points. In a coffee-cup calorimeter, 1.17 g NH_4NO_3 was mixed with 55.00 g water at an initial temperature 25.00 degree c. After dissolution of the salt, the final temperature of the calorimeter contents was 23.34 degree C. Assuming the solution has a heat capacity of 4.18 J/g middot degree C, and assuming no heat loss to the calorimeter, calculate the enthalpy of solution (Delta H_soln) for the dissolution of NH_4NO_3 in units of kJ/mol. Delta H_soln = k.J/mol In a coffee-cup calorimeter, 1.17 g NH_4NO_3 was mixed with 55.00 g water at an initial temperature 25.00 degree C. After dissolution of the salt, the final temperature of the calorimeter contents was 23.34 degree C. If the enthalpy of hydration for NH_4NO_3 is -630. kJ/mol, calculate the lattice energy of NH_4NO_3. Lattice energy = kJ/mol
Casey DurganLv2
7 Aug 2019