Calculate $\Delta \mathrm{H}^{\circ}{ }_{r \times n}$ for the reaction below given the enthalpies of formation.
$$
2 \mathrm{C}_{12} \mathrm{H}_{26}(\mathrm{~g})+37 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 24 \mathrm{CO}_{2}(\mathrm{~g})+26 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
$$
$$
\begin{array}{lc}
\underline{\Delta H^{\circ}}{ }^{\circ}(\mathrm{kJ} / \mathrm{mol}) & \
\mathrm{C}_{12} \mathrm{H}_{26}(\mathrm{~g}) & -70 \
\mathrm{CO}_{2}(\mathrm{~g}) & -394 \
\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) & -242
\end{array}
$$
$-17350 \mathrm{~kJ}$
$-12590 \mathrm{~kJ}$
$-21850 \mathrm{~kJ}$
$-15610 \mathrm{~kJ}$
$-567 \mathrm{~kJ}$

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Accepted Answer

***B*** ∻Key Concept∻ ⚹Hess's Law and Enthalpy of Formation⚹ ∻Explanation∻ ⚹The enthalpy change of a reaction ($\Delta H^\circ_{rxn}$) can be calculated using the standard enthalpies of formation ($\Delta H^\circ_f$) of the reactants and products. The formula is: $\Delta H^\circ_{rxn} = \sum \Delta H^\circ_f ( ext{products}) - \sum \Delta H^\circ_f ( ext{reactants})$.⚹◊What is the definition of enthalpy change in a chemical reaction, and how is it calculated based on the enthalpies of formation?⍭ Generate me a similar question◊

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