Sections | |||
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Internal Energy | 22 mins | 0 completed | Learn |

Calorimetry | 39 mins | 0 completed | Learn |

Hess's Law | 17 mins | 0 completed | Learn |

Enthalpy of Formation | 13 mins | 0 completed | Learn Summary |

End of Chapter 6 Problems | 52 mins | 0 completed | Learn |

Additional Practice |
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Units of Energy |

Endothermic & Exothermic Reactions |

Additional Guides |
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Enthalpy |

Solution: 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

Use the following equations

C (s) + O_{2 }(g) → CO_{2 }(g) ΔH ^{o} = 393.5 kJ

H_{2 }(g) + 1/2 O_{2 }(g) → H_{2}O (l) ΔH ^{o} = 285.8 kJ

2 C_{4}H_{10 }(g) + 13 O_{2} (g) → 8 CO_{2 }(g) + 10 H_{2}O (l) ΔH ^{o }= 5754.6 kJ

to calculate the heat formation, ΔH ^{o}_{f}, for butane.

4 C (s) + 5 H_{2} (g) → C_{4}H_{10} (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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