Do any of the following compounds exhibit london dispersion forces: CO, NH3, CO2, CH4, and H2?
Yes: all of them!
London dispersion forces arise from random movement of electrons within the electron cloud of an atom or molecule, causing said cloud to be distributed in such a way that it gives rise to an instantaneous dipole within the atom / molecule. This instantaneous dipole then induces temporary dipoles, appropriately called induced dipoles, in local atoms / molecules. The process continues throughout the crystal structure so that partial charges result in the implementation of a regular structure.
This applies to all molecular compounds and atoms, because electrons are able to move to continue redistributing the electron cloud within all atoms / molecules. London dispersion forces are the only things allowing certain monatomic gases such as argon, and diatomic gases like oxygen, to condense as you approach absolute zero.