Why does CO2 have higher boiling point than CO?

The intermolecular forces between $\ce{CO2}$ molecules are dispersion forces, while the forces between $\ce{CO}$ molecules are mostly dipole-dipole attraction forces. So, why does $\ce{CO2}$ have a higher boiling point than that of $\ce{CO}$?

• – Mithoron Jan 16 '16 at 18:40
• I don't think it answers my question. – Lyndt Jan 16 '16 at 18:53
• There are many other points on the scale from dipole-dipole interaction to dispersion forces. $\ce{CO}$ is a very weak dipole; on the other hand, $\ce{CO2}$ is a pretty strong quadrupole. – Ivan Neretin Jan 16 '16 at 19:23
• > the forces between COCO molecules are mostly dipole-dipole attraction forces. || Orientation of CO molecules in solid is random with weak preference of head-tail. This suggests that dispersion interactions dominates in CO solid. – permeakra Jan 17 '16 at 11:20
• Also the MW of $\ce{CO2}$ is about 57% greater than that of $\ce{CO}$ meaning that it will take considerably more energy to raise the kinetic energy of the heavier molecule to where it has the necessary surface escape velocity. – ron Jan 17 '16 at 19:38

$$\ce{CO2}$$ has 3 atoms involved in the molecule and is therefore larger than $$\ce{O2}$$ that has 2 atoms. Hence, $$\ce{CO2}$$ has a higher boiling / melting point compared to $$\ce{O2}$$. (Exception to this is water molecules.)