1. Determine the Temperature Change

* ΔT = Final Temperature - Initial Temperature

* ΔT = 22.4 °C - 25.3 °C = -2.9 °C

2. Determine the Mass of the Solution

* Assuming the density of the dilute solution is approximately 1 g/mL (close to the density of water), the mass of the solution is:

* Mass = Volume x Density = 100 mL x 1 g/mL = 100 g

3. Determine the Specific Heat Capacity of the Solution

* The specific heat capacity of a dilute ammonium nitrate solution is approximately the same as that of water, which is 4.184 J/(g·°C).

4. Calculate the Heat Absorbed

* The formula for calculating heat absorbed is:

* Q = m x c x ΔT

* Where:

* Q = heat absorbed (in Joules)

* m = mass of the solution (in grams)

* c = specific heat capacity (in J/(g·°C))

* ΔT = change in temperature (in °C)

* Plugging in the values:

* Q = 100 g x 4.184 J/(g·°C) x -2.9 °C

* Q = -1213.76 J

Important Note: The negative sign indicates that heat is *released* by the solution, not absorbed. This is because the temperature of the solution decreased.

Therefore, the solution released approximately 1213.76 Joules of heat.