Given the thermochemical equations 2C + 2O$_2$ \(\rightarrow\) 2CO$_2$ \(\Delta H = -786\) kJ 2CO$_2$ \(\rightarrow\) 2CO + O$_2$ \(\Delta H = +566\) kJ what is the \(\Delta H\) for this reaction? Please explicitly include the sign. 2C + O$_2$ \(\rightarrow\) 2CO kJ
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Step 1: We are given two thermochemical equations: 1) 2C + O2 -> 2CO2, H = -786 kJ 2) 2CO2 -> 2CO + O2, H = +566 kJ Show more…
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Explain the meaning of this thermochemical equation: $$\begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g) &+6 \mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H &=-904 \mathrm{kJ} / \mathrm{mol}\end{aligned}$$
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Using the following thermochemical equations $$ \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g})+\frac{7}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\ell) $$ $\Delta H=-1560 \mathrm{~kJ}$ $$ \begin{aligned} 2 \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\ell) \\ \mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\ell) & \Delta H=-2599 \mathrm{~kJ} \\ & \Delta H=-286 \mathrm{~kJ} \end{aligned} $$ calculate $\Delta H$ for $$ \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{~g}) \quad \Delta H=? $$
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