The standard enthalpies of formation of $C{O}_2\left(g\right)$ ${\text{, H}}_2\text{O}\left(\mathit{\text{l}}\right)$ and glucose (s) at $25^{\text{o}}C$ are $-\text{400 kJ}/\text{mol}$, $-\text{300 kJ}/\text{mol}$ and $-\text{1300 kJ}/\text{mol}$, respectively. The standard enthalpy combustion per gram of glucose at $25^{\text{o}}C$ is $\left(\Delta H_f^0=-1300kJmo{l}^{-}for\text{glucose}\right)$

Heat of combustion : It is the amount of heat evolved or absorbed (i.e. change in enthalpy) when one mole of the substance is completely burnt in air or oxygen.
Standard enthalpy of combustion of glucose reaction is given as
\(C _6 H _{12} O _{6(s)}+6 O _{2(g)} \rightarrow 6 CO _{2(g)}+6 H _2 O (l)\)
\(\Delta H _{ C }^{ o }=\Sigma_{\text {Product }} \Delta H _{ f }^{ o }-\Sigma_{\text {Reactant }} \Delta H _{ f }^{ o }\)
\(=\{6(-400)+6(-300)\}_{\text {Product }}-\{-1300\) \(\times ~1+6 \times 0\}_{\text {Reactant }}\)
\(=-2400-1800+1300=-2900 kJ mole ^{-1}\)
Molecular mass of glucose \(=72+12+96=180 g /\) mole
\(\Delta H _{ C }^{ o } /\) gram of glucose \(=\frac{-2900}{180}=-16.11 kJ / g\).