A 1.00 g sample of KCl is added to 20.0 gH2O in a styrofoam cup and stirred until dissolved. The temperature of the solution drops from 25.00 to 22.20∘C. Assume that the specific heat and density of the resulting solution are equal to those of water, 4.18 J/(g∘C) and 1.00 g/mL, respectively and assume that no heat is lost to the calorimeter itself, nor to the surroundings.
KCl(s)+H₂O(l)→KCl(aq)ΔH=?
Is this process endothermic or exothermic (circle the correct answer)?
