The dissolution of CaCl2(s) in water is exothermic, with ΔHsoln= - 81.3 kJ>mol. If you were to prepare a 1.00 m solution of CaCl2 beginning with water at 25.0 °C, what would the final temperature of the solution be in °C? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 J>1K g2.

The enthalpy of solution, ΔHsoln, refers to the heat change associated with the dissolution of a solute in a solvent. In this case, the dissolution of CaCl2 is exothermic, meaning it releases heat, which is indicated by a negative ΔHsoln value of -81.3 kJ/mol. This concept is crucial for understanding how the temperature of the solution changes as the solute dissolves.

Specific heat capacity is the amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius (or Kelvin). For this problem, it is given that the specific heat of both pure water and the resulting solution is 4.18 J/g·K. This property is essential for calculating the temperature change of the solution after the dissolution process.

Heat transfer during a chemical process, such as dissolution, affects the temperature of the system. The heat released by the dissolution of CaCl2 will increase the temperature of the water. By applying the formula q = mcΔT, where q is the heat absorbed or released, m is the mass, c is the specific heat, and ΔT is the change in temperature, one can determine the final temperature of the solution after the dissolution.