This data supports my hypothesis by showing that both reaction two and three lose energy and are exothermic. A deviation that occurred was a miscalculation during the experiment in which my partners and I measured the change in temperature at the wrong time which upon correction the data was not much different. The results follow the theories that have been approved. Some practical uses include energy synthesis as described above while theoretical uses are the energy of creatures and the energy provided by certain fuels as stated on chem wiki (Stephen lower and professor Emeritus 2007). There are no suggestions that come to mind for improving …show more content…
Then using the enthalpies found for reactions two and three I would find the enthalpy of reaction one the ideal reaction. Both reaction two and three are exothermic but reaction one is endothermic this is due to overall reaction one is building more bonds than it is breaking. The formula for finding the enthalpy of reaction one is as follows the change in enthalpy of reaction two combined with the inverse change in enthalpy of reaction three results in the enthalpy of reaction one. This indicates that the ideal reactions we are taught aren’t easily found so we must use Hess’s law and find the enthalpy of our ideal reaction using the two other reactions which occur in various