Chlorobenzene boils at 131.8C. Use Trouton's Rule to estimate deltaH of vaporization.
can you please show all the steps?
one more question please:
Calculate the delta S of vaporization for each of the liq: acetone, dimethyl ether, ethanol, octane, pyridine.
their delta H of vaporization are 29.1, 21.5, 38.6, 34.4, 35.1.
how do I do this????
1. Svap = about 87 J/mol*K = (delta Hvap/boiling pt). Substitute 131.8 for boiling point and calculate delta Hvap.
2. Use the same equation shown in 1 and substitute for delta Hvap and boiling point to determine delta Svap. The idea behind this question is to show that not ALL compounds obey Trouton's Rule, especially those that experience hydrogen bonding and/or those materials that tend to form dimers, trimers, or other polymeric forms.
how do you get 87J/molK
is the answer to question 1: 35.22 ( if temperature changed to K)?
To estimate deltaH of vaporization using Trouton's Rule, we need to know the boiling point of the compound and the boiling point of a reference compound.
Trouton's Rule states that the heat of vaporization (deltaHvap) for most nonpolar substances is approximately 88 J/mol·K or 20.9 cal/mol·K per degree of boiling point.
The boiling point of chlorobenzene is given as 131.8°C. We need to convert this temperature to Kelvin scale by adding 273.15:
131.8°C + 273.15 = 404.95 K
Now, we can use Trouton's Rule to estimate deltaHvap for chlorobenzene.
deltaHvap = (20.9 cal/mol·K) × (404.95 K)
deltaHvap ≈ 8448.195 cal/mol
Therefore, based on Trouton's Rule, the estimated deltaHvap for chlorobenzene is approximately 8448.195 cal/mol.