Question 11.1: calculating a Vapor pressure Using the clausius–clapeyron Eq...
Calculating a Vapor Pressure Using the Clausius–Clapeyron Equation
The vapor pressure of ethanol at 34.7 °C is 100.0 mm Hg, and the heat of vaporization of ethanol is 38.6 kJ/mol. What is the vapor pressure of ethanol in millimeters of mercury at 65.0 °C
IDENTIFY
Known | Unknown |
∆H_{vap} = 38.6 kJ/mol | Vapor pressure at 65.0 °C (P_{2}) |
Vapor pressure at 34.7 °C (P_{1} = 100.0 mm Hg) | |
T_{1} = 34.7 °C | |
T_{2} = 65.0 °C |
STRATEGY
Use the rearranged form of the Clausius–Clapeyron equation that enables us to calculate the vapor pressure of the liquid at any other temperature if we know the heat of vaporization and the vapor pressure at one temperature. Convert temperature to Kelvin and ∆H_{vap} to units of joules.
ln(\frac{P_{1}}{P_{2}})=\frac{\Delta H_{vap}}{R}(\frac{1}{T_{2}}-\frac{1}{T_{1}})
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