# Copy of 3.01 Heats of Reaction.pdf - Hess’s Law - Heats of...

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Hess’s Law - Heats of ReactionUsing the Standard values ofΗ°f, calculate the heats of reaction,ΔΗ°rxn, or heats of formation,ΔΗ°fAll answers must include the intermediate steps with the formation reaction from the elements and theirmanipulation to form the overall reaction.For #1-6, the equation:∆Hrxn° = Σn∆Hf°productsΣn∆Hf°reactantsCANNOT BE USED.1.C6H6(l)+15/2O2(g)6 CO2(g)+3 H2O (g)2.2 HNO3(aq) +NO (g)3 NO2(g)+H2O (l)3.C2H2(g)+C2H6(g)2 C2H4(g)4.PbO2(s)+CO (g)PbO (s)+CO2(g)5.Al2(SO4)3 (s)+3 H2O (l)Al2O3 (s)+3 H2SO4(aq)6.3 SO2(s)+2 HNO3(aq) +2 H2O (l)3 H2SO4(aq)+2 NO (g)7.Given that ∆H°rxn=- 1196.0 kJ for the following, calculate the ∆H°ffor ClF3(g).2 ClF3(g)+2 NH3(g)N2(g)+6 HF (g)+Cl2(g)8.Given that ∆H°rxn=- 52.3 kJ for the following, calculate the ∆H°ffor HNO2(g).HNO2(g)+1/2 O2(g)HNO3(aq)9.Given that ∆H°rxn=- 386.2 kJ for the following, calculate the ∆H°ffor Fe(CO)5(g).Fe2O3(s)+13 CO (g)2 Fe(CO)5(g)+3 CO2(g)10.Given that ∆H°rxn=+ 47.2 kJ for the following, calculate the ∆H°f

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