Chemical energetics: describe question

The standard enthalpy change of formation of ethanol, $\Delta H_f^\circ[\ce{C2H5OH(l)}]$, cannot be measured directly by calorimetry. The following standard enthalpy changes of combustion, $\Delta H_c^\circ$, are known:

$$\ce{C(s) + O2(g) -> CO2(g)} \quad \Delta H_c^\circ = -394\ \text{kJ mol}^{-1}$$ $$\ce{H2(g) + 1/2 O2(g) -> H2O(l)} \quad \Delta H_c^\circ = -286\ \text{kJ mol}^{-1}$$ $$\ce{C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l)} \quad \Delta H_c^\circ = -1367\ \text{kJ mol}^{-1}$$

Describe how Hess's law can be applied to determine $\Delta H_f^\circ[\ce{C2H5OH(l)}]$. Include in your description how the energy cycle is constructed and the steps used to combine the data.