Explain how the Kekulé model of benzene is contradicted by the hydrogenation enthalpies of ethene and benzene

The Kekulé model of benzene consists of a 6 membered ring with 3 double bonds. This would imply a hydrogenation enthalpy very similar to that of ethene, since double bonds react with hydrogen in a similar statement way, however we find that the enthalpy is less positive than expected. This is due to the delocalisation of the electrons in the pi bonds spreading the electron density across the ring, leading to benzene being more stable than predicted, as there is less electron density in an aromatic bond than a normal C=C bond. (Also I would draw the resonance structures of the Kekulé model demonstrating the delocalisation)