1. The problem statement, all variables and given/known data In this investigation, you mix .5g of Mg(s) with 115mL HCl. You measure the temperature change which turns out to be 25.5 degrees C. The equation is as follows: Mg + 2HCL --> MgCl2 + H2 Use the specific heat of water (c=4.184) to find the heat of formation. What is the temperature change of 1mol of MgCl2? 2. Relevant equations Q=cm(t2-t1) Kind of basic algebra that I think I'm getting wrong. Or maybe I'm using the wrong variables. 3. The attempt at a solution This problem uses the specific heat of water. This means that we must use the mass of water as well (1mol = 18g). Q=4.184(18g)(t2-t1) I am having trouble with the temperature change. Mg is the limiting reactant. Therefore: .5g Mg (mol/24.31g) = .021mol Mg (mol MgCl2/mol Mg) = .021mol MgCl2 .021mol MgCl2 (95.21g MgCl2/mol MgCl2) = 1.99941 ~2.00g MgCl2 Therefore: (25.5C/2.00g MgCl2) * 95.21g MgCl2 = 1214C This answer however, isn't correct. Am I supposed to use the masses of water instead?