The normal boiling point of ethanol(C 2 H 5 OH) is 78.5\'C. Using the informatio

Question

The normal boiling point of ethanol(C2H5OH) is 78.5'C. Using the informationfrom Thermodynamic Data at 1 atm and 25'C, and the followinginformation: H'f(C2H5OH(g)) = -234.38 kJ/mol a) Determine the enthalpy of vaporization of ethanol. b) Use the Clausius-Clapeyron equation to estimate the vaporpressure of ethanol at 25'C. The normal boiling point of ethanol(C2H5OH) is 78.5'C. Using the informationfrom Thermodynamic Data at 1 atm and 25'C, and the followinginformation: H'f(C2H5OH(g)) = -234.38 kJ/mol a) Determine the enthalpy of vaporization of ethanol. b) Use the Clausius-Clapeyron equation to estimate the vaporpressure of ethanol at 25'C.

Explanation / Answer

(a)   Using Troutons rule we can calculate thevapH        Troutons rule :  vapH / Tb =85JK^-1mol^-1                       vapH = 85JK^-1mol^-1 * (78.5 + 273)K                                        = 29877.5 Jmol^-1 (b)    Hint: Use the below equation to solve for vapour pressure ofethanol at 25'C        ln(P* / P) = +(vapH/ R )[(1/T) - (1/T*)]

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