Using Hess's Law to Determine the Enthalpy of a Reaction: Report Sheet Part 1: Determine the Enthalpy for Reaction \#1 Molarity of HCl : 1 Average Hreaction= Standard Deviation = Part 2: Determine the Enthalpy for Reaction \#2 Molarity of HCl : Port 2: Hrin=molgxn462.511J/mol Average Hreaction= Standard Deviation = 1. Are the experimental reactions tested in this experiment endothermic or exothermic? Support your answer from the data collected in the experiment. 2. Fill in the enthalpies for reactions \#1-3 using the experimental values you calculated for reaction #1 and 2. Then use Hess's law to find the enthalpy of reaction #4. Reaction \#1: MgO(s)+2HCl(aq)MgCl2(aq)+H2O(l),H1= Reaction \#2: Mg(s)+2HCl(aq)MgCl2(aq)+H2(g),H2= Reaction \#3: H2(g)+21O2(g)H2O(l),H3=g l l/mul Reaction \#4: Mg (s)+21O2(g)MgO(s),H4= exprimentul Guspter 6017ks/mol 3. Calculate the percent error for the enthalpy of reaction \#4 by comparing the experimentally determined value versus the standard accepted value using the \% error formula below. %Error=acceptedexperimentalaccepted100 4. Give two possible sources of experimental error. (Experimental error refers to the uncertainties associated with experimental limitations, and not necessarily mistakes made by the experimentalist or mistakes in calculations.)