Question
Consider the reaction$2 \mathrm{ClF}_{3}(g)+2 \mathrm{NH}_{3}(g) \longrightarrow \mathrm{N}_{2}(g)+6 \mathrm{HF}(g)+\mathrm{Cl}_{2}(g)$$\Delta H^{\circ}=-1196 \mathrm{~kJ}$Calculate $\Delta H_{\mathrm{f}}^{\circ}$ for $\mathrm{ClF}_{3}(g)$.
Step 1
The reaction is: \[ 2 \mathrm{ClF}_{3}(g) + 2 \mathrm{NH}_{3}(g) \longrightarrow \mathrm{N}_{2}(g) + 6 \mathrm{HF}(g) + \mathrm{Cl}_{2}(g) \] with \(\Delta H^{\circ} = -1196 \mathrm{~kJ}\). Show more…
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Use the reaction $$\begin{aligned} 2 \mathrm{ClF}_{3}(g)+2 \mathrm{NH}_{3}(g) \longrightarrow \mathrm{N}_{2}(g)+6 \mathrm{HF}(g)+\mathrm{Cl}_{2}(g) & \\ \Delta H^{\circ}=-1196 \mathrm{kJ} \end{aligned}$$ to calculate $\Delta H_{f}^{\circ}$ for $\mathrm{ClF}_{3}(g)$.
Consider the reaction $$2 \mathrm{ClF}_{3}(g)+2 \mathrm{NH}_{3}(g) \longrightarrow \mathrm{N}_{2}(g)+6 \mathrm{HF}(g)+\mathrm{Cl}_{2}(g)$$ Calculate $\Delta H_{\mathrm{f}}^{\circ}$ for $\mathrm{ClF}_{3}(g)$.
Given the following data $$\begin{aligned} 2 \mathrm{ClF}(g)+\mathrm{O}_{2}(g) & \longrightarrow \mathrm{Cl}_{2} \mathrm{O}(g)+\mathrm{F}_{2} \mathrm{O}(g) & & \Delta H=167.4 \mathrm{kJ} \\ 2 \mathrm{ClF}_{3}(g)+2 \mathrm{O}_{2}(g) & \longrightarrow \mathrm{Cl}_{2} \mathrm{O}(g)+3 \mathrm{F}_{2} \mathrm{O}(g) & & \Delta H=341.4 \mathrm{kJ} \\ 2 \mathrm{F}_{2}(g)+\mathrm{O}_{2}(g) & \longrightarrow 2 \mathrm{F}_{2} \mathrm{O}(g) & & \Delta H=-43.4 \mathrm{kJ} \end{aligned}$$ calculate $\Delta H$ for the reaction $$\mathrm{ClF}(g)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{ClF}_{3}(g)$$
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