Which of the following equations represents a reaction that provides the heat of formation of ${\mathrm{CH}}_3\mathrm{Cl}$?

Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction:

${\mathrm{TiCl}}_4\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to {\mathrm{TiO}}_2\left(\mathrm{g}\right)+4\mathrm{HCl}\left(\mathrm{g}\right)$

$∆{\mathrm{H}}_{\mathrm{f}}^{\mathrm{o}}{\mathrm{TiCl}}_4\left(\mathrm{g}\right)=-763.2 \mathrm{kJ}/\mathrm{mole}$

$∆{\mathrm{H}}_{\mathrm{f}}^{\mathrm{o}}{\mathrm{TiO}}_2\left(\mathrm{g}\right)=-944.7 \mathrm{kJ}/\mathrm{mole}$

$∆{\mathrm{H}}_{\mathrm{f}}^{\mathrm{o}}{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)=-241.8 \mathrm{kJ}/\mathrm{mole}$

$∆{\mathrm{H}}_{\mathrm{f}}^{\mathrm{o}}\mathrm{HCl}\left(\mathrm{g}\right)=-92.3 \mathrm{kJ}/\mathrm{mole}$

 The heats of formation of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ are $-394\mathrm{kJ}/\mathrm{mole}$ and $-285.8\mathrm{kJ}/\mathrm{mole}$ respectively. Using the data for the following combustion reaction, calculate the heat of formation of ${\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)$.

${\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\to 3{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

$∆\mathrm{H}°=-2221.6 \mathrm{kJ}$

The heats of formation of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ and ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ are $-394\mathrm{kJ}/\mathrm{mole}$ and $-285.8\mathrm{kJ}/\mathrm{mole}$ respectively. Using the data for the following combustion reaction, calculate the heat of formation of ${\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)$.

$2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\to 4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

$∆\mathrm{H}°=-2601\mathrm{kJ}$

Using the following information calculate the heat of formation of ${\mathrm{CH}}_4$.

${\mathrm{CH}}_4\left(\mathrm{g}\right)+2{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

$∆\mathrm{H}°=-890.4\mathrm{kJ}$

$∆{\mathrm{H}}_{\mathrm{f}}^{°}{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}=-393.5\mathrm{kJ}/\mathrm{mole}$

$∆{\mathrm{H}}_{\mathrm{f}}^{°}{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}=-285.9\mathrm{kJ}/\mathrm{mole}$

The heat of formation of ${\mathrm{CO}}_2\left(\mathrm{g}\right)$ is $-394\mathrm{kJ}/\mathrm{mole}$ and that of ${\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ is $-286\mathrm{kJ}/\mathrm{mole}$. The heat of combustion of ${\mathrm{C}}_2{\mathrm{H}}_4$ is $-1412\mathrm{kJ}/\mathrm{mole}$. What is the heat of formation of ${\mathrm{C}}_2{\mathrm{H}}_4$?

${\mathrm{C}}_2{\mathrm{H}}_4\left(\mathrm{g}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

What amount of heat energy $\left(\mathrm{kJ}\right)$ is released in the combustion of $12.0 \mathrm{g}$ of ${\mathrm{C}}_3{\mathrm{H}}_4$? (Atomic weights: $\mathrm{C}=12.01,\mathrm{H}=1.008,\mathrm{O}=16.00$).

${\mathrm{C}}_3{{\mathrm{H}}_4}_{\left(\mathrm{g}\right)}+4{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\to 3{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}+2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{l}\right)}$

$∆\mathrm{H}°=-1939.1\mathrm{kJ}$