**Clausius-Clapeyron Equation:**

$\overline{){\mathbf{ln}}\mathbf{}{\mathbf{P}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{\Delta H}}_{\mathbf{vap}}}{\mathbf{R}}\mathbf{\left(}\frac{\mathbf{1}}{\mathbf{T}}\mathbf{\right)}}$

where: **P** = vapor pressure

The vapor pressure of a substance is measured over a range of temperatures. A plot of the natural log of the vapor pressure versus the inverse of the temperature (in Kelvin) produces a straight line with a slope of −3.44×10^{3} K .

Find the enthalpy of vaporization of the substance.

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