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Internal Energy | 22 mins | 0 completed | Learn |

Calorimetry | 39 mins | 0 completed | Learn |

Thermochemical Equation | 6 mins | 0 completed | Learn Summary |

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 |

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Enthalpy |

Solution: The following sequence of reactions occurs in the commercial production of aqueous nitric acid:4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(l) ΔH = −907 kJ2NO(g) + O2(g) ⟶ 2NO2(g)

Solution: The following sequence of reactions occurs in the commercial production of aqueous nitric acid:4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(l) ΔH = −907 kJ2NO(g) + O2(g) ⟶ 2NO2(g)

The following sequence of reactions occurs in the commercial production of aqueous nitric acid:

4NH_{3}(g) + 5O_{2}(g) ⟶ 4NO(g) + 6H_{2}O(l) ΔH = −907 kJ

2NO(g) + O_{2}(g) ⟶ 2NO_{2}(g) ΔH = −113 kJ

3NO_{2} + H_{2}O(l) ⟶ 2HNO_{3}(aq) + NO(g) ΔH = −139 kJ

Determine the total energy change for the production of one mole of aqueous nitric acid by this process.

To find the ΔHrxn, we need to combine the three reactions where we should be getting HNO_{3} as product

However, the problem is asking for the energy needed to produce 1 mole of HNO_{3}, and in the given 3rd reaction, we have 2 moles of HNO_{3}

We will be dividing the final ΔH calculated by 2 to get the energy needed for every 1 mol HNO_{3} produced

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Use the standard reaction enthalpies given below t...

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