Data Analysis

Graph displaying inverse of temperature versus the natural log of pressure

(Ethanol is supposed to be the green line, and the acetone is the blue line)

Graph displaying time versus temperature

Table 1: Heat of Vaporization determined for ethanol and acetone

The heat of vaporization was found using the equation:

Acetone:

Ethanol:

Conclusion:

The purpose of this lab is to understand how intermolecular interactions affect physical properties.  In order to do this, ethanol and acetone were heated to a certain temperature, separately, then the pressure was observed as they cooled to a certain temperature.  The heat of vaporization was then calculated using the Clausius-Clapeyron equation, and the slopes taken from the graphs. The heat of vaporization for Acetone was 20,286 J/mol, while Ethanol's heat of vaporization was 24,942 J/mol.   The lower heat of vaporization for Acetone demonstrates the weaker intermolecular interactions between the Acetone molecules, while the higher heat of vaporization for Ethanol demonstrates the stronger intermolecular interactions between the Ethanol molecules.  Some sources of error could of been from not knowing whether the Ethanol and Acetone were boiling.  If the substances were not boiling enough, the recording of pressure as it cooled would not of been accurate.