Oooh, assuming there are no scientific reference/tables, that's not necessarily straight forward. You're going to be experts in thermodynamics by studying that you know
E.g. let's see, Myrcene's vapor pressure is 2.09 mm Hg at 25 deg C for example. This is less than water whose vapor pressure is 23.7 mm Hg at 25 deg C. This tends to indicate that water is more volatile than Myrcene at around room temperature when the pressure and humidity is the same, for instance.
alpha-pinene has a vapor pressure of 4.75 mm Hg at 25 deg C. This indicates that it is more volatile than Myrcene but less volatile than water.
The higher the vapor pressure, the higher the evaporation will be. And, it is not linear with temperature. As the temperature increases, the rate of evaporation will increase likely in an exponential fashion (I think). In most cases, looking at the boiling point (e.g. in the table) gives you a general idea as to the volatility and rate of evaporation at temperatures that are less than boiling.
From the vapor pressures, you can get a general idea of how fast something will evaporate. But, even though water is more volatile, there is most certainly much more water to evaporate away than the terpenes.
e.g. complicated, me thinks.
So, going more complicated, then:
Calculating actual rates of evaporation, the starting point would be the latent heat of vaporization aka enthalpy of vaporization or evaporation which is the amount of energy (enthalpy) that must be added to a liquid substance, to transform a given quantity of the substance into a gas.
Here is how it can be calculated for water:
A different or more complex substance complicates it further. It is not a simple thing to figure out but there may be some short-cuts. I'll look around but this might be something a bit off-topic and suggesting something that may not be the primary cause in this op. But it is an interesting question in general.
Is there more info in that cool table such as vapor pressure, cannacrab?
Sorry for the rambling...