8. Thermochemistry

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.

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.

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

Calculate the enthalpy of the reaction 2NO(g) + O₂(g) → 2NO₂(g) given the following reactions and enthalpies of formation: 12N₂(g) + O₂(g) → NO₂(g), δH^∘_a=33.2 kJ 12N₂(g) + 12O₂(g) → NO(g), δH^∘_b=90.2 kJ

What is the isobaric heat of combustion for ethane, C₂H₆(g), in kJ per mole of ethane at 298.15 k?

How much energy is required to decompose 765 g of PCl₃

What is the heat of combustion of ethane, C₂H₆, in kilojoules per mole of ethane? Enthalpy of formation values can be found in this list of thermodynamic properties.