Asked by Jake
I was wondering if anyone could possible help me with this homework question?
<b>The normal boiling point for acetone is 56.5 degrees C. At an elevation of 5300 ft the atmospheric pressure is 630. torr. What would be the boiling point of acetone (deltahvap = 32.0 kJ/mol) at this elevation? What would be the vapor pressure of acetone at 25.0 degrees C at this elevation?</b>
<b>The normal boiling point for acetone is 56.5 degrees C. At an elevation of 5300 ft the atmospheric pressure is 630. torr. What would be the boiling point of acetone (deltahvap = 32.0 kJ/mol) at this elevation? What would be the vapor pressure of acetone at 25.0 degrees C at this elevation?</b>
Answers
Answered by
DrBob222
Use the Clausius-Clapeyron equation.
760 torr is the pressure at the normal boiling point of 56.5. Don't forget that T1 and T2 must be in Kelvin, delta H vap must be in J and R = 8.314 J/mol*K.
760 torr is the pressure at the normal boiling point of 56.5. Don't forget that T1 and T2 must be in Kelvin, delta H vap must be in J and R = 8.314 J/mol*K.
Answered by
Carmen
thanks!
Answered by
Carmen
Whoops sorry, wrong one.
Answered by
Jake
Thank you!