How do you do this chemistry lab problem?

Question

The equation relating approximate barometric pressure (P, in torr) to altitude(h, in m) is at room T:

lnP = 6.63-(h8000)

Diethyl ether, CH3CH2OCH2CH3, a common organic solvent has a normal boiling point at 34.6 degrees C (and thus vapor pressure of 760 torr at 34.6 C). at 20 degrees C, it has a vapor pressure of 440 torr. At what approximate altitude will diethyl ether boil at 20 C? Where on the earth would it be a problem to keep this solvent liquid?

Answer 1

It looks like your pressure equation should read
ln(P) = 6.63 - h/8000
Then
h = 8,000(6.63 - ln(P))
When P = 440
h = 4,346 m (14,258 ft.)
This elevation is to be found on some of the higher mountain peaks and ranges.