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17 Nov 2019
Consider the following reactions:
2 C8H18 (l) + 25 O2(g) â 16 CO2(g) + 18H2O(g) ÎHo =-10920.0 kJ/mol
C(diamond) (s) + O2(g) â CO2(g) ÎH= -373.39 kJ/mol
C(diamond) (s) + O2(g) â CO2(g) ÎHo = -395.39 kJ/mol
1/2 C(diamond) (s) â 1/2 C(graphite) (s) ÎH= -0.945 kJ/mol
1/2 O2 + H2(g) â H2O(l) ÎHo = -285.8 kJ/mol
H2O(g) â 1/2 O2 + H2(g) ÎHo = 241.8 kJ/mol
Using these reactions in conjunction with Hess' Law to determine the enthalpy of formation of octane at standard state conditions.
Consider the following reactions:
2 C8H18 (l) + 25 O2(g) â 16 CO2(g) + 18H2O(g) ÎHo =-10920.0 kJ/mol
C(diamond) (s) + O2(g) â CO2(g) ÎH= -373.39 kJ/mol
C(diamond) (s) + O2(g) â CO2(g) ÎHo = -395.39 kJ/mol
1/2 C(diamond) (s) â 1/2 C(graphite) (s) ÎH= -0.945 kJ/mol
1/2 O2 + H2(g) â H2O(l) ÎHo = -285.8 kJ/mol
H2O(g) â 1/2 O2 + H2(g) ÎHo = 241.8 kJ/mol
Using these reactions in conjunction with Hess' Law to determine the enthalpy of formation of octane at standard state conditions.
Reid WolffLv2
17 Nov 2019
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