Hello there, I am supposed to experimentally determine (with the use of a calorimeter) the overall heat of reaction per mole of calcium metal in two cases: 1. When I mix HCL, calcium and water in that order. 2. When I mix water, calcium and HCL in that order. In each case, I am supposed to treat the overall reaction as a single process and determine a ΔH for the two-step process using my determined overall change in temperature. I've purposefully left out the provided numerical values, hoping to understand more where to start than to solve the actual problem at the moment; however I can provide them if desired. From what I understand, I'm supposed to basically sum up the overall reaction in an equation and that both ways should theoretically result in the release of the same amount of energy... but how on earth would I go about calculating the heat of reaction using the overall temperature change? I will mention that we are provided with the following: 1. Mass of the solution 2. Initial and final temperature 3. Mass of each reagent and the calorimeter itself 4. Heat capacity of the calorimeter Depressing as it is, I'm fairly lost and any information would be appreciated, thanks. NOTE: My current attempt revolves around treating the solution as having a heat capacity similar to water, and having the ΔH = CmΔT(water) + CΔT (calorimeter). I don`t know if it`s very appropriate to assume such a thing however and would like to see if there`s any other ideas.