Question
The standard heat of formation of ethylene, $\mathrm{C}_{2} \mathrm{H}_{4}(g)$, is $+52.284 \mathrm{~kJ} \mathrm{~mol}^{-1} .$ Calculate the $\mathrm{C}=\mathrm{C}$ bond energy in this molecule.
Step 1
We need two moles of gaseous carbon atoms and four moles of gaseous hydrogen atoms to form one mole of ethylene. The energy required to create these atoms can be found in table 18.3. Let's denote the energy required to create one mole of gaseous carbon atoms as Show more…
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The standard enthalpy of combustion of ethene gas $\left[\mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g})\right]$ is $-1411.1 \mathrm{kJ} / \mathrm{mol}$ at $298 \mathrm{K} .$ Given the following enthalpies of formation, calculate $\Delta H_{f}^{\circ}$ for $\mathrm{C}_{2} \mathrm{H}_{4}(g)$ $$\begin{array}{ll} \mathrm{CO}_{2}(g) & -393.5 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{H}_{2} \mathrm{O}(l) & -285.8 \mathrm{kJ} / \mathrm{mol} \end{array}$$
The standard enthalpy of combustion of ethene gas, $\mathrm{C}_{2} \mathrm{H}_{4}(g)$ is $-1411.1 \mathrm{kJ} / \mathrm{mol}$ at $298 \mathrm{K}$. Given the following enthalpies of formation, calculate $\Delta H_{\mathrm{f}}^{\circ}$ for $\mathrm{C}_{2} \mathrm{H}_{4}(g)$. $$\begin{array}{ll}\mathrm{CO}_{2}(g) & -393.5 \mathrm{kJ} / \mathrm{mol} \\\mathrm{H}_{2} \mathrm{O}(l) & -285.8 \mathrm{kJ} / \mathrm{mol}\end{array}$$
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