What amount of energy (in $KJ$) is released in the combustion of $5.8\, g$ of $C_4H_{10}\,(g)$?
$2 C_4H_{10}(g) + 13 O_2(g) \to 8 CO_2(g) + 10 H_2O(l)$; $\Delta H^o = -5756\, KJ$

Given that the bond energy of hydrogen-hydrogen bond is $436 \ kJ/mol$,that of hydrogen-oxygen bond is $464 \ kJ/mol$,and those in oxygen molecules $496 \ kJ/mol$,what is the approximate heat of reaction for $2H_2 + O_2 \longrightarrow 2H_2O$ ? .....$kJ/mol$

If the enthalpy of formation of $N_2O$ is $82 \, kJ \, mol^{-1}$,calculate the resonance energy of $N_2O$ in $kJ \, mol^{-1}$.
$N \equiv N \, (946 \, kJ \, mol^{-1}); \, N = N \, (418 \, kJ \, mol^{-1})$
$O = O \, (498 \, kJ \, mol^{-1}); \, N = O \, (607 \, kJ \, mol^{-1})$

According to Hess's Law,the enthalpy change of a reaction depends on which of the following?

Combustion of glucose takes place according to the equation,$C_6H_{12}O_6 + 6O_2 \to 6CO_2 + 6H_2O$,$\Delta H = -72 \ kcal$. How much energy will be required for the production of $1.6 \ g$ of glucose? (Molecular mass of glucose $= 180 \ g/mol$)

The heat of formation of $CO_{(g)}$ and $CO_{2(g)}$ are $-26.4 \ kcal$ and $-94.0 \ kcal$ respectively. The heat of combustion of carbon monoxide will be $... \ kcal$.