CHEMISTRY COMMUNITY

can the delta h of sublimation be calculated by adding the delta h of melting with the delta h of vaporization? Or does it take a totally separate path? But because delta H is a state function, shouldn't it be the case that sublimation's enthalpy change is the same as the enthalpy change of melting and then vaporizing something? If this is the case, why consider sublimation as it's own thing at all?

Yes, the enthalpy of sublimation can be calculated by adding up the enthalpy of fusion (melting) and the enthalpy of vaporization. This is because enthalpy is a state function, so it can be added up like this, since sublimation is going from a solid directly to a gas, you can just add the enthalpies of the 2 phase changes, from solid to liquid, and from liquid to gas.