For the reaction $H_{2(g)} + I_{2(g)} \rightarrow 2HI_{(g)}; \Delta H = 12.40 \, Kcal$,the heat of formation of $HI$ is ....... $Kcal$.

Explain the standard enthalpy of formation.

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

Which of the following equations represents the standard enthalpy of formation of $CH_4$?

The heats of combustion of yellow phosphorus and red phosphorus are $-9.91 \, kJ$ and $-8.78 \, kJ$ respectively. The heat of transition for the conversion of yellow phosphorus to red phosphorus will be ...... $kJ$?

Calculate $\Delta_r H$ $(kJ \ mol^{-1})$ of the following reaction:
$C_2H_5OH_{(l)} + \frac{7}{2}O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$

Molecule	$\Delta_f H^0 (kJ \ mol^{-1})$
$C_2H_5OH_{(l)}$	$-280$
$CO_{2(g)}$	$-400$
$H_2O_{(l)}$	$-290$