Sections | |||
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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 values for the enthalpy of reaction are given for two reactions below
Mg(s) + Na 2CO3(s) → 2 Na(s) + MgCO 3(s) ΔH rxn = 317.1 kJ
Mg(s) + 2 NaF(s) → 2 Na(s) + MgF 2(s) ΔH rxn = 35.6 kJ
Based on this information, what is the value for ΔH rxn for the reaction
MgCO3(s) + 2 NaF(s) → Na 2CO3(s) + MgF2(s)
a. + 352.7 kJ
b. + 281.5 kJ
c. + 245.9 kJ
d. - 281.5 kJ
e. - 352.7 kJ

The values for the enthalpy of reaction are given for two reactions below

Mg(s) + Na _{2}CO_{3}(s) → 2 Na(s) + MgCO _{3}(s) ΔH _{rxn} = 317.1 kJ

Mg(s) + 2 NaF(s) → 2 Na(s) + MgF _{2}(s) ΔH _{rxn} = 35.6 kJ

Based on this information, what is the value for ΔH _{rxn} for the reaction

MgCO_{3}(s) + 2 NaF(s) → Na _{2}CO_{3}(s) + MgF_{2}(s)

a. + 352.7 kJ

b. + 281.5 kJ

c. + 245.9 kJ

d. - 281.5 kJ

e. - 352.7 kJ

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