Problem: A liquid has a ΔH°vap of 35.5 kJ/mol and a boiling point of 122°C at 1.00 atm. What is its vapor pressure at 113°C?

FREE Expert Solution

Use the Clausius-Clapeyron Equation:

lnP2P1=-HfusionR[1T2-1T1]ln(P21 atm)=-(-35.5 kJmol)(1x103 J1 kJ)8.314 Jmol K[1113+273.15 K-1122+273.15 K]ln(P21 atm)=-35500 Jmol8.314 Jmol K(5.898x10-5 K-1)ln(P21 atm)=-0.25185P21 atm = 0.7773 atm

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A liquid has a ΔH°vap of 35.5 kJ/mol and a boiling point of 122°C at 1.00 atm. What is its vapor pressure at 113°C?

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.