I don't really get this problem
It's about vapor pressure, and I dunno if I'm supposed to use the Ideal Gas Law because volume of the original liquid doesn't affect the vapor pressure at equilibrium.
A certain compound has a normal melting point of 41 degrees C & a normal boiling pont of 123 degrees C. The triple point is 39 degrees C and 85 mm Hg. The vapor pressure of the compound at 50 degrees is 120 mm Hg.
If 4.60 g of the compound (molar mass of 20.0 g/mol) is placed in a 2.00 L flask at 50 degrees C, what is/are the physical state(s) of the compound in the flask? Show by calculation.
I dont really kno how to calculate it. I'd appreciate if u guys can help.