(Solved): Determine the vapor pressure of chloroform, in \( \mathrm{mmHg} \), at \( 31^{\circ} \mathrm{C} \). ...

Determine the vapor pressure of chloroform, in \( \mathrm{mmHg} \), at \( 31^{\circ} \mathrm{C} \). Chloroform normally boils at \( 61.7^{\circ} \mathrm{C} \) under atmospheric conditions and has a heat of vaporization of \( 31.4 \mathrm{~kJ} / \mathrm{mol} \). Your answer should be numerical and neglect units (e.g., if you calculate \( 3.5 \) \( \mathrm{mmH} \mathrm{g} \) then input 3.5).