We are asked to use Trouton’s rule to estimate the enthalpy of vaporization of chloroform.

$\overline{){\mathbf{\u2206}}{{\mathbf{S}}}_{{\mathbf{vap}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{\u2206}{\mathbf{H}}_{\mathbf{vap}}}{{\mathbf{T}}_{\mathbf{b}}}}$

Where:

ΔS_{vap} = 85 J/mol-K

Calculate ΔH_{vap}

Given:

ΔS_{vap} = 85 J/mol-K

T_{b} = 61.2°C + 273.15 = 334.35 K

The boiling point of chloroform, CHCl _{3}, is 61.2°C. Use Trouton’s rule to estimate the enthalpy of vaporization of chloroform.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Entropy concept. You can view video lessons to learn Entropy. Or if you need more Entropy practice, you can also practice Entropy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Arman's class at UTSA.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.