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青州's Question
Chemistry
Posted 2 months ago

Calculate ΔHr×n\Delta \mathrm{H}^{\circ}{ }_{r \times n} for the reaction below given the enthalpies of formation.
2C12H26( g)+37O2( g)24CO2( g)+26H2O(g)
2 \mathrm{C}_{12} \mathrm{H}_{26}(\mathrm{~g})+37 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 24 \mathrm{CO}_{2}(\mathrm{~g})+26 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})

ΔH(kJ/mol)C12H26( g)70CO2( g)394H2O(g)242
\begin{array}{lc}
\underline{\Delta H^{\circ}}{ }^{\circ}(\mathrm{kJ} / \mathrm{mol}) & \\
\mathrm{C}_{12} \mathrm{H}_{26}(\mathrm{~g}) & -70 \\
\mathrm{CO}_{2}(\mathrm{~g}) & -394 \\
\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) & -242
\end{array}

17350 kJ-17350 \mathrm{~kJ}
12590 kJ-12590 \mathrm{~kJ}
21850 kJ-21850 \mathrm{~kJ}
15610 kJ-15610 \mathrm{~kJ}
567 kJ-567 \mathrm{~kJ}
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Answer from Sia
Posted 2 months ago
B
Key Concept
Hess's Law and Enthalpy of Formation
Explanation
The enthalpy change of a reaction (ΔHrxn\Delta H^\circ_{rxn}) can be calculated using the standard enthalpies of formation (ΔHf\Delta H^\circ_f) of the reactants and products. The formula is: ΔHrxn=ΔHf(products)ΔHf(reactants)\Delta H^\circ_{rxn} = \sum \Delta H^\circ_f (\text{products}) - \sum \Delta H^\circ_f (\text{reactants}).

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