Calorimetry Lab

In this graph the results is about what we expected, which is a big amount of heat given off. In observing the graph the distance between reaction 1 and reaction 2 shows the total amount of heat given off which is the combination of 1&2 in comparison to room temperature that the water was originally at. Through the experiment there was a lot of question as to if we were doing it right, were we swirling the solution around enough, did we open the top right so heat would not escape, did we collect the data at the right time? Now looking back I see that many of the things that our group did defiantly altered our data, making me question the reliability of the data we collected. The first reaction was CaCO3(s) + 2HCL(aq)------- CaCl2(aq) + H20(l) + CO2(g) and the second reaction that was given was Ca(OH)2(s) + 2HCl(aq)-------CaCl2(aq) + 2H2o(l) combined gave off about 57 degrees Celsius going into a system (Calomitery and Hess’s Law). I personally recognized this, knowing the type of equations that were given for this experiment. However, I have not recognized anything excessively wrong when comparing the two reactions with the data that I

Common since will invade ones thoughts when doing this experiment knowing that the overall purpose is to find the total product of heat, one should keep the experimentation isolated as much as possible from the outside room temperate. This is why we used a lid for the experiment, the lid slows the speed of the reaction going to room temperature (Calorimetry and Hess’s Law). One of the things that I was very skeptical about when doing the experiment was when we took the lid off in order to put the substances into the solution. Heat escaping would give the q a smaller change of enthalpy change of our two reactions as a result giving us false