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A 2.00 g sample of KCl is added to 35.0 g H2O in a styrofoam cup...

A 2.00 g sample of KCl is added to 35.0 g H2O in a styrofoam cup and stirred until dissolved. The temperature of the solution drops from 24.8 to 21.6 ˚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) ∆H = ? a) Is the reaction endothermic or exothermic? b) What is the heat of solution of KCl expressed in kilojoules per mole of KCl?

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