Correct! The given compounds are arranged in order of increasing boiling point.

CH3-CH3 (ethane) has the lowest boiling point as it is a simple nonpolar molecule with weak London dispersion forces.

CH3-CH2Cl (chloroethane) has a higher boiling point than ethane due to the presence of a polar covalent bond between carbon and chlorine, leading to stronger dipole-dipole interactions.

C4H10 (butane) has a higher boiling point than chloroethane due to its larger size and increased number of electrons, resulting in stronger London dispersion forces.

CH2=CH-CH2-CH3 (1-butene) has the highest boiling point among the given compounds as it has the presence of a double bond, leading to stronger intermolecular forces of attraction compared to the other compounds.