Find the enthalpy of formation for the following chemical reaction.

2Al (s) + Fe₂O₃ (s) --> Al₂O₃ (s) + 2Fe (s)

Find the enthalpy change that occurs over the following two-step equations.

2 H₂ (g) + O₂ (g) --> 2 H₂O (l) ΔH = -572 kJ

2 H2O2 (l) --> 2 H2 (g) + 2 O2 (g) ΔH = 376 kJ

Find the change in enthalpy over the following two-step equations.

N₂ (g) + O₂ (g) --> 2 NO (g) ΔH = 180kJ

2 NO (g) + O₂ (g) --> 2 NO₂ ΔH = -112kJ

How much energy would it take to condense 4.9 moles of C₂H₅OH?

How much energy is required to turn 7.3 moles of NH₃ from a solid to a liquid?