Determine the temperature change that occurs when 10.6 g of potassium perchlorate (KClO4) is dissolved in enough water to make 104.8 mL of solution, given that the enthalpy of dissolution is -55.5 kJ/mol.

Convert the volume of the solution from milliliters to liters, as the specific heat capacity is typically given in terms of liters. Use the conversion: \( 1 \text{ mL} = 0.001 \text{ L} \).

Assume the specific heat capacity of the solution is similar to that of water, which is approximately 4.18 J/g°C. Calculate the mass of the solution using the density of water (1 g/mL), and then use the formula: \( q = m \cdot c \cdot \Delta T \), where \( q \) is the heat absorbed or released, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the temperature change.