1. The problem statement, all variables and given/known data When 0.612 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 100C is observed. Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC. (Note: Pay attention to significant figures. Do not round until the final answer.) The molar heat of reaction, H rxn, for the reaction of Ca(s) + 2H+(aq) => Ca2+(aq) + H2 (g) 2. Relevant equations Q=mc[tex]\Delta[/tex]T 3. The attempt at a solution All I know is that mc[tex]\Delta[/tex]T is used... Our professor hasn't taught us how to do this yet so that's about all I know. Would I divide Q by the number of moles formed?