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Unformatted text preview: solid = 1.84 J/g o C, S liquid = 4.18 J/g o C, q fusion = 6.01 kJ/mol) Name: 2 Part II: Diborane. II.1 (19 points) Diborane (B 2 H 6 ) is a colorless gas that can ignite spontaneously at room temperature. In the late 1940s there was much interest in using mixtures with diborane as rocket fuels. However, it was realized that diborane also forms boron oxides that reduced performance. The reaction of elemental B (s) and H 2 (g) does not generate diborane. Calculate the standard enthalpy of formation of diborane using the following measured reactions: The standard enthalpy of formation of B 2 O 3 (s) is -1271.9 kJ/mol B 2 O 3 (s). The standard enthalpy of formation of H 2 O (g) is -241.8 kJ/mol H 2 O (g). The standard enthalpy change of the following reaction is: B 2 H 6 (g) + 3 O 2 (g) B 2 O 3 (s) + 3 H 2 O (g) H o = -2032.9 kJ/mol B 2 O 3 (s)...
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This note was uploaded on 07/09/2008 for the course CHEM 342132 taught by Professor Davis during the Spring '08 term at Cornell University (Engineering School).
- Spring '08