The vapor pressure of a volatile liquid was plotted againsttemperature according

Question

The vapor pressure of a volatile liquid was plotted againsttemperature according to the Clausius-Clapeyron equation (lnP vs. 1/T). It was found that the data fit theequation of a straight line of the form y = 6446.6x+ 19.539. What is the normal boiling point of the liquid?

I thought that if y=0 you could solve for x and take the inverseof that but it didn't work. Does anyone else know how to do it.

The vapor pressure of a volatile liquid was plotted againsttemperature according to the Clausius-Clapeyron equation (lnP vs. 1/T). It was found that the data fit theequation of a straight line of the form y = 6446.6x+ 19.539. What is the normal boiling point of the liquid?

I thought that if y=0 you could solve for x and take the inverseof that but it didn't work. Does anyone else know how to do it.

Explanation / Answer

You have to work in mmHg units. It should have been specified inthe question. normal pressure = 760mmHg, and if you solve it, it gives you theresult of 500K to the boiling temperature.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.