Calculate ΔHrsn for the reaction: CH4( g)+4 Cl2(g) ⟶CCl4(g)+4 HCl(g) Use the following reactions

step 1 In this question we're going to be applying Hec's law which states that the total enthalpy chang

Calculate ΔHrsn for the reaction: CH4( g)+4 Cl2(g)...

Calculate $\Delta H_{\mathrm{rsn}}$ for the reaction: $$ \mathrm{CH}_{4}(\mathrm{~g})+4 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g)+4 \mathrm{HCl}(g) $$ Use the following reactions and given $\Delta H$ 's. $$ \begin{array}{cc} \mathrm{C}(s)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{4}(g) & \Delta H=-74.6 \mathrm{~kJ} \\ \mathrm{C}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g) & \Delta H=-95.7 \mathrm{~kJ} \\ \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g) & \Delta H=-92.3 \mathrm{~kJ} \end{array} $$

Calculate $\Delta H_{\mathrm{rsn}}$ for the reaction:
$$
\mathrm{CH}_{4}(\mathrm{~g})+4 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g)+4 \mathrm{HCl}(g)
$$
Use the following reactions and given $\Delta H$ 's.
$$
\begin{array}{cc}
\mathrm{C}(s)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{4}(g) & \Delta H=-74.6 \mathrm{~kJ} \\
\mathrm{C}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(g) & \Delta H=-95.7 \mathrm{~kJ} \\
\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{HCl}(g) & \Delta H=-92.3 \mathrm{~kJ}
\end{array}
$$

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Key Concepts

Manipulation of Thermochemical Equations

Manipulation of thermochemical equations involves reversing, scaling, and adding or subtracting individual reaction equations to derive a target overall reaction. Each mathematical operation on a reaction's equation must be accompanied by the same operation on its associated enthalpy change, ensuring accurate calculation of the overall enthalpy change through the additive property of energy.

Enthalpy Change of Reaction

The enthalpy change of a reaction represents the heat absorbed or released under constant pressure during a chemical reaction. It is an extensive property that can be determined or estimated using standard enthalpies of formation, bond energies, or by applying Hess’s Law through the combination and manipulation of thermochemical equations.

Hess’s Law

Hess’s Law states that the total enthalpy change for a reaction is the same, no matter how many steps the reaction is carried out in. This principle allows the calculation of an unknown reaction enthalpy by algebraically combining other reactions with known enthalpies, emphasizing that enthalpy is a state function and independent of the reaction pathway.

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