The ΔHf^0 of TiI3(s) is -328 kJ / mol and the ΔH^∘ for the reaction 2 Ti(s)+3 I2(g) ⟶2 TiI3(s)

step 1 In this question we've been asked to determine the enthalpy change of reaction, the standard ent

The ΔHf^0 of TiI3(s) is -328 kJ / mol and the ΔH^∘ for the...

The $\Delta H_{\mathrm{f}}^{0}$ of $\mathrm{TiI}_{3}(s)$ is $-328 \mathrm{~kJ} / \mathrm{mol}$ and the $\Delta H^{\circ}$ for the reaction $2 \mathrm{Ti}(s)+3 \mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{TiI}_{3}(s)$ is $-839 \mathrm{~kJ} .$ Calculate the $\Delta H$ of sublimation of $\mathrm{I}_{2}(s)$, which is a solid at $25{ }^{\circ} \mathrm{C}$.

The $\Delta H_{\mathrm{f}}^{0}$ of $\mathrm{TiI}_{3}(s)$ is $-328 \mathrm{~kJ} / \mathrm{mol}$ and the $\Delta H^{\circ}$ for the reaction $2 \mathrm{Ti}(s)+3 \mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{TiI}_{3}(s)$ is $-839 \mathrm{~kJ} .$ Calculate the $\Delta H$
of sublimation of $\mathrm{I}_{2}(s)$, which is a solid at $25{ }^{\circ} \mathrm{C}$.

Key Concepts

Standard Enthalpy of Formation

This is the enthalpy change when one mole of a compound forms from its constituent elements in their standard states. It serves as a reference for calculating reaction enthalpies using Hess's law by combining formation enthalpies of reactants and products.

Hess's Law

A principle stating that the total enthalpy change for a chemical reaction is the same regardless of the pathway taken. This allows one to calculate unknown enthalpy changes by combining known reaction steps, as enthalpy is a state function.

Sublimation

The phase transition from a solid to a gas. The enthalpy of sublimation is the amount of energy required for this transition, and it is critical to include in thermochemical calculations when substances change phase between their standard states.

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