Based on the molar enthalpies calculated for Experiment 2 and Experiment 3, you can now use Hess’s law to write out a series of reactions that will sum up to the reaction of the decomposition of ammonium chloride NH4Cl(s) ? NH3(g) + HCl(g) In addition to the molar enthalpies from Experiment 2 and 3, you will also need to include the following reactions which account for the enthalpy change when HCl and NH3 change state: A) NH3 (g) -> NH3 (aq) (dH = -34,640 J/mol)
B) HCl (g) -> HCl (aq) (dH = -75,140 J/mol)
C) NH4Cl (s)-> NH4Cl (aq) (dH= 18065 J/mol)
D) HCL(s) + NH3(aq) ->NH4Cl(aq) (dH = 53,180 j/mol)