Combining Bond Enthalpies and Enthalpies of Formation
You can combine this data. You just need to find a sensible reaction cycle, and you have to make sure the temperatures (usually 298 K) match. 

To give a simple example, consider $\ce{CO2(g)}$. 

What is the $\ce{CO}$ bond enthalpy $\mathrm{\epsilon_{C=O}}$in $\ce{CO2(g)}$? 

It is one half of the enthalpy for the reaction 

$$\ce{ CO2(g)-&gt;C(g) + 2O(g)}~~~~~\mathrm{\Delta  H^\circ = 2 \epsilon_{C=O}}$$

The enthalpy of formation of $\ce{CO2(g)}$ is equal to the enthalpy of combustion of graphite:

$$\ce{C(s) + O2(g) -&gt; CO2(g)} ~~~~~~\mathrm{\Delta _f H^\circ = -393.51}\pu{kJ mol^{-1}}$$

The heat of formation of $\ce{C(g)}$ is: 

$$\ce{C(s) -&gt; C(g) }~~~~~~\mathrm{\Delta _f H^\circ = 716.68}\pu{kJ mol^{-1}}$$

We also need a value of the $\ce{OO}$ bond enthalpy in $\ce{O2}$: 

$$\ce{O_2(g) -&gt; 2O(g) }~~~~\mathrm{\Delta  H^\circ = \epsilon_{O=O} =  498.3}\pu{kJ mol^{-1}}$$

Adding things up we obtain $\mathrm{\epsilon_{C=O}}$: 

$$\mathrm{\epsilon_{C=O}} = \frac12(393.51+716.68+498.3)\pu{kJ mol^{-1}= 804.2 kJ mol^{-1}}$$