when the vapor pressure of a particular substance at a given temperature changes, then that change is reflected in a shift in the liquid-gas boundary on a phase diagram, correct?

So, for example, if the Pvap increases, then the liquid-gas boundary would shift closer to the y axis resulting in a lower boiling point?

Thus, the liquid-gas boundary is essentially the Pvap vs. T graph. However, when the Pvap changes due to changes in intermolecular forces, we are working on a different curve, correct?

Question

when the vapor pressure of a particular substance at a given temperature changes, then that change is reflected in a shift in the liquid-gas boundary on a phase diagram, correct?

So, for example, if the Pvap increases, then the liquid-gas boundary would shift closer to the y axis resulting in a lower boiling point?  

Thus, the liquid-gas boundary is essentially the Pvap vs. T graph. However, when the Pvap changes due to changes in intermolecular forces, we are working on a different curve, correct?