The enthalpy of combustion (∆Hc) of aluminum borohydride, Al(BH4)3(l), was measured to be -4138.4 kJ/mol [Rulon and Mason, J. Am. Chem. Soc.,73, 5491 (1951)]. The combustion reaction for this compound is given by
Al(BH4)3(l) + 6 O2(g) → ½ Al2O3(s) + 3/2 B2O3(s) + 6 H2O(l)
Given the following additional data, calculate the enthalpy of formation of Al(BH4)3(g).
Substance | Property |
Al2O3(s) | ∆Hf = -1669.8 kJ/mol |
B2O3(s) | ∆Hf = -1267.8 kJ/mol |
H2O(l) | ∆Hf = -285.84 kJ/mol |
Al(BH4)3(l) | ∆Hvap = 30.125 kJ/mol |
∆Hf = ___ kJ/mol
- 343.365 kJ/mol
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