a. 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 3.42 g of NH₄ClO₄(s) are dissolved in 113.80 g of water, the temperature of the solution drops from 25.74 to 23.56 C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.68 J/C. Based on the student's observation, calculate the enthalpy of dissolution of NH₄ClO₄(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. H_dissolution = kJ/mol

b. 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 5.05 g of NH₄Br(s) are dissolved in 109.90 g of water, the temperature of the solution drops from 25.34 to 23.30 C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/C. Based on the student's observation, calculate the enthalpy of dissolution of NH₄Br(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. H_dissolution = kJ/mol

c. 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 8.84 g of CsCl(s) are dissolved in 101.80 g of water, the temperature of the solution drops from 22.54 to 20.08 C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.89 J/C. Based on the student's observation, calculate the enthalpy of dissolution of CsCl(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. H_dissolution = kJ/mol