Methanethiol has a vapor pressure of 429 torr at −25 ∘c and a normal boiling point of 6.0 ∘c. find δhvap for methanethiol.

Naturally, this type of thermodynamic problem calls for a formula. In this case, we need the Clausius-Clapeyron equation which is shown in the attached picture. Take note of the given units shown in the legend.

Tb = 6 + 273 = 279 K
T0 = -25 + 273 = 248 K
P0 = 429 torr * 101.325 kPa/706 torr = 61.57 kPa

Applying the equation,

279 = {[8.314(ln61.57 - ln101.325)/ΔHvap] + 1/248}⁻¹
Use a scientific calculator to find ΔHvap.
ΔHvap = 9,244.25 J/mol

1= c 2= a or d3 = idk sorry 4= c5= c

What is the question