Calculate enthalpy change (in kJ) when 2 moles of liquid acetic acid undergoes dissociation into ${\mathrm{CH}}_4\left(\mathrm{g}\right)$ and
${\mathrm{CO}}_2\left(g\right)$ from the following data :$\mathrm{\Delta }{H}_{\mathrm{vap}}\left[{\mathrm{CH}}_3\mathrm{COOH}\right]\left(l\right)=50 \mathrm{kJ}/\mathrm{mole}$ 
Resonance energy of ${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{g}\right)=-50 \mathrm{kJ}/\mathrm{mole}$
Resonance energy of ${\mathrm{CO}}_2\left(\mathrm{g}\right)=-25 \mathrm{kJ}/\mathrm{mole}$
Bonding energy $(\mathrm{kJ}/\mathrm{mole}):\mathrm{C}-\mathrm{H}=400;\mathrm{C}-\mathrm{O}=350$:
$\begin{array}{l}\mathrm{O}=\mathrm{O}=500\\ \mathrm{C}-\mathrm{C}=350;\mathrm{O}-\mathrm{H}=450;\mathrm{C}=\mathrm{O}=800;\mathrm{H}-\mathrm{H}=400\end{array}$