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## Homework Statement

Liquid X boils at 127C, at a pressure of 10.6*10^5 Pa. Its enthalpy of vaporization is 5000 J/mol. At what temperature will it boil if the pressure is raised to 1.08*10^5 Pa?

## Homework Equations

[itex]\frac{dT}{dP}=\frac{l}{T(v_{B}-v_{A})}[/itex]

## The Attempt at a Solution

It seems so simple, but I don't know what to do about the specific volumes in the denominator. I have tried saying that because the second phase is a gas v_B>>v_A, neglecting v_A, then using the ideal gas equation to substitute for v_B = V_B/N = K*T_B/P_B.

I get T_B (final temp.) as about 4*10^13 K. Which has got to be way way off.

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