Use the value of enthalpy you determined for CaCl2 to calculate what quantity of salt will be needed to make a chemical hot pack. Assume using 100 g (100 mL) of water and changing the temperature from 25 °C to 60 °C. Show all calculations.

The Fundamentals of Calorimetry

Student Name

• Date
• Purpose
• Procedure
• Experimental Data

Table 1

Insert graph of the data from Data Table 1, plotting temperature vs. time, and use the Y intercept to find the temperature at time 0 when the two volumes of water are mixed.

Table 2

Table  3

Report data with correct units.  Show calculations below the table

Show calculations for first column:

• Moles of salt
• Heat released/absorbed by the solution
• Heat released/absorbed by the calorimeter
• Enthalpy of solution (J)
• Enthalpy of solution (kJ)
• Molar Enthalpy of solution
• Average molar enthalpy of solution

Insert graphs of ΔT vs. grams of salt for NH₄Cl

Lab Questions

2. What sort of relationship exists between the temperature change and the mass of the salt dissolved? Explain your answer.
3. The actual molar enthalpy of solution for calcium chloride is -81.3 kJ/mol, whereas the molar enthalpy of solution of ammonium chloride is 14.8 kJ/mol. Calculate the percent error of your results. Show the calculations.
4. Use the value of enthalpy you determined for CaCl₂ to calculate what quantity of salt will be needed to make a chemical hot pack. Assume using 100 g (100 mL) of water and changing the temperature from 25 °C to 60 °C. Show all calculations.
5. Use the graph you drew for NH₄Cl to determine the amount of salt needed to make a chemical cold pack. Assume using 100 g (100 mL) of water. The temperature should go down to 3.0 °C from a room temperature of 25 °C. Show all calculations.
6. Suggest practical ways in which the calorimeter or lab protocol could be improved to decrease percent errors.