AP Chemistry
6.9 Hess’s Law
6.6 Introduction to Enthalpy of Reaction
Industrial production of titanium metal begins with the high-temperature carbochlorination of titanium dioxide, represented by the balanced chemical equation below.
\[ \text{TiO}_2(s) + 2\,\text{C}(s) + 2\,\text{Cl}_2(g) \rightarrow \text{TiCl}_4(l) + 2\,\text{CO}(g) \]
A thermochemist uses the following standard enthalpies of reaction at \(298\text{ K}\) to determine the overall enthalpy change of this synthesis:
\[ \text{Reaction 1: } \text{Ti}(s) + 2\,\text{Cl}_2(g) \rightarrow \text{TiCl}_4(l) \quad \Delta H^\circ_1 \]
\[ \text{Reaction 2: } \text{Ti}(s) + \text{O}_2(g) \rightarrow \text{TiO}_2(s) \quad \Delta H^\circ_2 \]
\[ \text{Reaction 3: } \text{CO}(g) \rightarrow \text{C}(s) + \dfrac{1}{2}\,\text{O}_2(g) \quad \Delta H^\circ_3 \]
Based on the reactions provided, which of the following expressions correctly represents the value of \(\Delta H^\circ_{\text{rxn}}\) for the carbochlorination process?
\[ \text{TiO}_2(s) + 2\,\text{C}(s) + 2\,\text{Cl}_2(g) \rightarrow \text{TiCl}_4(l) + 2\,\text{CO}(g) \]
A thermochemist uses the following standard enthalpies of reaction at \(298\text{ K}\) to determine the overall enthalpy change of this synthesis:
\[ \text{Reaction 1: } \text{Ti}(s) + 2\,\text{Cl}_2(g) \rightarrow \text{TiCl}_4(l) \quad \Delta H^\circ_1 \]
\[ \text{Reaction 2: } \text{Ti}(s) + \text{O}_2(g) \rightarrow \text{TiO}_2(s) \quad \Delta H^\circ_2 \]
\[ \text{Reaction 3: } \text{CO}(g) \rightarrow \text{C}(s) + \dfrac{1}{2}\,\text{O}_2(g) \quad \Delta H^\circ_3 \]
Based on the reactions provided, which of the following expressions correctly represents the value of \(\Delta H^\circ_{\text{rxn}}\) for the carbochlorination process?
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