Adding 5.00 g of to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 17.5 °C to 15.1 °C. Calculate the enthalpy change for dissolving in water in kJ/mol. Assume the solution (whose mass is 145.0 g) has a specific heat capacity of 4.2 J/g · K. (Cold packs take advantage of the fact that dissolving ammonium nitrate in water is an endothermic process.) A cold pack uses the endothermic enthalpy of a solution of ammonium nitrate. Enthalpy change = kJ/mol

11.8 g of a soluble ionic compound is dissolved in 91.6 mL of water in a coffee-cup calorimeter, and the temperature of the solution changes from 24.80°C to 29.14°C. Assume the water has a density of 1.00 g/mL and that the total mass of the solution has the specific heat of water (4.186 J/g.K). Calculate the enthalpy change for the dissolution of this substance in kJ.

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 0.90 g of CaCl2(s) are dissolved in 102.10 g of water, the temperature of the solution increases from 22.90 to 24.48 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.79 J/°C.Based on the student's observation, calculate the enthalpy of dissolution of CaCl2(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water.ΔHdissolution = kJ/mol

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