Use Hess's Law to calculate \( \Delta G^{\circ}{ }_{r \times n} \) using the following information: \[ \begin{array}{cl} \mathrm{ClO}(g)+\mathrm{O}_{3}(g) \rightarrow \mathrm{Cl}(g)+2 \mathrm{O}_{2}(g) & \Delta \mathrm{G}^{\circ}{ }_{\mathrm{rxn}}=? \\ 2 \mathrm{O}_{3}(g) \rightarrow 3 \mathrm{O}_{2}(g) & \Delta \mathrm{G}_{\mathrm{rxn}}^{\circ}=+489.6 \mathrm{~kJ} \\ \mathrm{Cl}(g)+\mathrm{O}_{3}(g) \rightarrow \mathrm{ClO}(g)+\mathrm{O}_{2}(g) & \Delta \mathrm{G}_{[\times \mathrm{xn}}=-34.5 \mathrm{~kJ} \end{array} \] Your answer should have four significant figures and include either a positive or negative sign. The free energy of the target reaction is type your answer... kJ
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The target reaction is: \[ \mathrm{ClO}(g) + \mathrm{O}_{3}(g) \rightarrow \mathrm{Cl}(g) + 2 \mathrm{O}_{2}(g) \] And the given reactions are: Show more…
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Calculate Use Hess's law to determine $\Delta H$ for the reaction $N O(g)+O(g)+0(g) \rightarrow$ $N O_{2}(g) \Delta H=?$ given the following reactions. Show your work. $\begin{array}{l}{\mathrm{O}_{2}(\mathrm{g}) \rightarrow 20(\mathrm{g}) \Delta \mathrm{H}=+495 \mathrm{kJ}} \\ {2 \mathrm{O}_{3}(\mathrm{g}) \rightarrow 30_{2}(\mathrm{g}) \Delta \mathrm{H}=-427 \mathrm{kJ}} \\ {\mathrm{NO}(\mathrm{g})+\mathrm{O}_{3}(\mathrm{g}) \rightarrow \mathrm{NO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \Delta \mathrm{H}=-199 \mathrm{kJ}}\end{array}$
Given the data $$\begin{aligned} \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}(g) & \Delta H=+180.7 \mathrm{kJ} \\ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) & \Delta H=-113.1 \mathrm{kJ} \\ 2 \mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 2 \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) & \Delta H=-163.2 \mathrm{kJ} \end{aligned}$$ use Hess's law to calculate $\Delta H$ for the reaction $$\mathrm{N}_{2} \mathrm{O}(g)+\mathrm{NO}_{2}(g) \longrightarrow 3 \mathrm{NO}(g)$$
Use Hess's law to determine $\Delta_{r} H^{\circ}$ for the reaction $\mathrm{C}_{3} \mathrm{H}_{4}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow \mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{g}),$ given that $\mathrm{H}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ $$\Delta_{\mathrm{r}} H^{\circ}=-285.8 \mathrm{kJ} \mathrm{mol}^{-1}$$ $\mathrm{C}_{3} \mathrm{H}_{4}(\mathrm{g})+4 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow 3 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(1)$ $$\Delta_{\mathrm{r}} H^{\circ}=-1937 \mathrm{kJ} \mathrm{mol}^{-1}$$ $\mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{g})+5 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow 3 \mathrm{CO}_{2}(\mathrm{g})+4 \mathrm{H}_{2} \mathrm{O}(1)$ $$\Delta_{\mathrm{r}} H^{\circ}=-2219.1 \mathrm{kJ} \mathrm{mol}^{-1}$$
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