Question
For $\mathrm{SF}_{6}(g), \Delta H^{\circ}=-1096 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Use the data in Table 18.3 to calculate the average $S-\mathrm{F}$ bond energy in $\mathrm{SF}_{6}$
Step 1
Step 1: We start by writing the formation reaction for $\mathrm{SF}_{6}$: \[S(s) + 3F_{2}(g) \rightarrow SF_{6}(g)\] Show more…
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Estimate the average S-F bond energy in $\mathrm{SF}_{6}$. The values of standard enthalpy of formation of $\mathrm{SF}_{6}(\mathrm{~g}), \mathrm{S}(\mathrm{g})$ and $\mathrm{F}(\mathrm{g})$ are $:-1100,275$ and $80 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.
Thermodynamics
Topic 2 : Thermochemistry
Gaseous hydrogen sulfide, $\mathrm{H}_{2} \mathrm{~S},$ has $\Delta H_{\mathrm{f}}^{\circ}=$ $-20.15 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Use the data in Table 18.3 to calculate the average $S-\mathrm{H}$ bond energy in this molecule.
Carbon disulfide, $\mathrm{CS}_{2}$, has the Lewis structure $\ddot{S}=C=\ddot{S},$ and for $C S_{2}(g), \Delta H_{\mathrm{f}}^{\circ}=+115.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$ Use the data in Table 18.3 to calculate the average $\mathrm{C}=\mathrm{S}$ bond energy in this molecule.
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