Identify the molecule for which the enthalpy of atomization $\left(\Delta_{a} H^{\ominus}\right)$ and bond dissociation enthalpy $\left(\Delta_{BOND} H^{\ominus}\right)$ are not equal.

Which factor affects the heat of reaction in the Kirchhoff equation?

The enthalpy change during a reaction does not depend on .......

Given that $C_{(g)} + 4H_{(g)} \to CH_{4(g)}; \Delta H = -166 \ kJ$,the bond energy of the $C-H$ bond will be....$kJ/mole$.

If the enthalpy of combustion of carbon is $-393 \, kJ \, mol^{-1}$,calculate the heat produced by the combustion of $1 \, g$ of carbon in $kJ$.

For strong acid and strong base neutralisation,the net chemical change is $H^{+} + OH^{-} \longrightarrow H_2O_{(l)}$; $\Delta_r H^{\circ} = -55.84 \ kJ \ mol^{-1}$. If the enthalpy of neutralisation of $CH_3COOH$ by $NaOH$ is $-49.86 \ kJ \ mol^{-1}$,then the enthalpy of ionisation of $CH_3COOH$ is: