Calculate the standard enthalpy of hydrogenation of ethyne to ethene in kJ/mol using enthalpies of combustion data.
Added by Sebastian J.
Step 1
First, we need to know the reactions for the combustion of ethyne (C2H2), ethene (C2H4), and hydrogen (H2). The combustion reactions are as follows: C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l) ΔHc1 = -1300 kJ/mol C2H4(g) + 3 O2(g) → 2CO2(g) + 2H2O(l) Show more…
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The standard enthalpies of combustion of ethyne $\left[\mathrm{C}_{2} \mathrm{H}_{2}(g)\right], \mathrm{C}(s),$ and $\mathrm{H}_{2}(g)$ are $-1299.6,-393.5,$ and $-285.9 \mathrm{kJ} / \mathrm{mol},$ respectively. Use this information to calculate the standard enthalpy of formation of ethyne.
The enthalpies of combustion of ethene, ethane, and hydrogen are -1390 kJ/mol, -1550 kJ/mol, and -286 kJ/mol respectively. Use the data to calculate the enthalpy of the reaction with hydrogen to form ethane.
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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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