Problem: Use the following equations C (s) + O2 (g) → CO2 (g)                                                  ΔH     o = 393.5 kJ H2 (g) + 1/2 O2 (g) → H2O (l)                                           ΔH     o = 285.8 kJ 2 C4H10 (g) + 13 O2 (g) → 8 CO2 (g) + 10 H2O (l)           ΔH o = 5754.6 kJ to calculate the heat formation, ΔH of, for butane. 4 C (s) + 5 H2 (g)  →  C4H10 (g) A.  125.7 kJ B. -5880.3 kJ C. -5862.3 kJ D. -5075.3 kJ E. -251.4 kJ    

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Problem Details

Use the following equations

C (s) + O(g) → CO(g)                                                  ΔH     o = 393.5 kJ
H(g) + 1/2 O(g) → H2O (l)                                           ΔH     o = 285.8 kJ
2 C4H10 (g) + 13 O2 (g) → 8 CO(g) + 10 H2O (l)           ΔH = 5754.6 kJ

to calculate the heat formation, ΔH of, for butane.
4 C (s) + 5 H2 (g)  →  C4H10 (g)

A.  125.7 kJ
B. -5880.3 kJ
C. -5862.3 kJ
D. -5075.3 kJ
E. -251.4 kJ

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