Representing Energy Changes: Draw the potential energy diagram for the reaction in question 4. PE NH4+(aq) + NO3-(aq) ΔH = +22.9 kJ NH4NO3(s) Reaction Progress Create the 2 forms of thermochemical equations that we learned in class. NH4NO3(s) NH4+(aq) + NO3-(aq) ΔH = +22.9 kJ NH4NO3(s) + 22.9 kJ NH4+(aq) + NO3-(aq) Hess’s Law: Calculate the enthalpy for the following reaction using the given thermochemical equations. CS2(l) + 3O2(g) CO2(g) + 2SO2(g) = ? ΔH C(s) + O2(g) CO2(g) = -393.5 kJ x 1 ΔH S(s) + O2(g) SO2(g) = -296.8 kJ x 2 ΔH C(s) + 2S(s) CS2(l) = +87.9 kJ x (-1) ΔH C(s) + O2(g) CO2(g) = -393.5 kJ ΔH 2S(s) + 2O2(g) 2SO2(g) = -593.6 kJ ΔH CS2(l) C(s) + 2S(s) = -87.9 kJ ΔH CS2(l) + 3O2(g) CO2(g) + 2SO2(g) = -1075 kJ ΔH
Representing Energy Changes: Draw the potential energy diagram for the reaction in question 4. PE NH4+(aq) + NO3-(aq) ΔH = +22.9 kJ NH4NO3(s) Reaction Progress Create the 2 forms of thermochemical equations that we learned in class. NH4NO3(s) NH4+(aq) + NO3-(aq) ΔH = +22.9 kJ NH4NO3(s) + 22.9 kJ NH4+(aq) + NO3-(aq) Hess’s Law: Calculate the enthalpy for the following reaction using the given thermochemical equations. CS2(l) + 3O2(g) CO2(g) + 2SO2(g) ΔH = ? C(s) + O2(g) CO2(g) ΔH = -393.5 kJ x 1 S(s) + O2(g) SO2(g) ΔH = -296.8 kJ x 2 C(s) + 2S(s) CS2(l) ΔH = +87.9 kJ x (-1) C(s) + O2(g) CO2(g) ΔH = -393.5 kJ 2S(s) + 2O2(g) 2SO2(g) ΔH = -593.6 kJ CS2(l) C(s) + 2S(s) ΔH = -87.9 kJ CS2(l) + 3O2(g) CO2(g) + 2SO2(g) ΔH = -1075 kJ