The vapor pressure of hexane (C6H14) is 40.0 Torr at -2.30 °C and 100.0 Torr at 15.8 °C. [1 atm = 760 Torr =?
The vapor pressure of hexane (C6H14) is 40.0 Torr at -2.30 °C and 100.0 Torr at 15.8
°C. [1 atm = 760 Torr = 760 mm Hg]. Calculate the enthalpy of vaporization of hexane
within this temperature range.
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use the clausius clapeyron equation
ln(P1/P2) = (-dHvap / R) x (1/T1 - 1/T2)
P1 = 40.0 torr
P2 = 100.0 torr
R = 8.315 J/moleK
T1 = -2.30+273.15K = __K
T2 = 15.8+273.15 = __K
solve for dHvap and calculate
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