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8. Thermochemistry

Enthalpy of Formation

8. Thermochemistry

Enthalpy of Formation

Multiple Choice
Using the standard enthalpies of formation, calculate ΔH°rxn for the reaction: CaO(s) + CO2(g) → CaCO3(s). Given: ΔH°f [CaO(s)] = -635.1 kJ/mol, ΔH°f [CO2(g)] = -393.5 kJ/mol, ΔH°f [CaCO3(s)] = -1206.9 kJ/mol.
Multiple Choice
Using standard thermodynamic data, calculate ΔH°_rxn for the following:
2 C₂H₂ (g) + 5 O₂ (g) → 4 CO₂ (g) + 2 H₂O (l)
Multiple Choice
The oxidation of ammonia is illustrated by the following equation:
4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)
Calculate the enthalpy of reaction,ΔH_Rxn, based on the given standard heats of formation.
Multiple Choice
Consider the following equation:
2 ClF₃(g) + 2 NH₃(g) → 1 N₂(g) + 6 HF (g) + 6 Cl₂(g)ΔH_rxn = –1196 kJ
Determine the standard enthalpy of formation for chlorine trifluoride, ClF₃.
Multiple Choice
Find ΔH_rxn for the following reaction:
N₂ + 2 O₂ → 2 NO₂
Based on the following data.
2 NO → N₂ + O₂ ΔH = −180 kJ
2 NO + O₂ → 2 NO₂ ΔH = −112 kJ