The vapor pressure of ethanol is 400 mmhg at 63.5°c. its molar heat of vaporization is 39.3 kj/mol. what is vapor pressure of ethanol, in mmhg, at 34.9°c? (2 point clausius clapperon)

- The pressure of ethanol would be 109 mmHg.

Solution:- This problem is based on Clausius clapeyron equation--

Given, = 63.5 + 273 = 336.5 K

= 34.9 + 273 = 307.9 K

= 400 mmHg

= ?

= 39.3 kJ/mol = 39300 J/mol

R = 8.314 J/mol.K

Let's plug in the values in the equation and do the calculations.

= 1.30

On taking anti ln to both sides...

=

= 3.67

= 400/3.67

= 109 mmHg