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April 20, 2014

April 20, 2014

Posted by **Angel** on Sunday, February 26, 2012 at 6:47pm.

Calculate where the number 40.67 came from.

Use the Clapeyron-Clausisus equation. Assuming that delta H vap does not change with temperature, this equation relates the change in vapor pressure and temperature to a substance's enthalpy of vaporization (R is the molar mass constant). Use this relationship and the fact that delta H vap of water at 25 degrees Celsius is 43.99 kJ/mol to calculate the vapor pressure of water at 5,25,50, and 95 degrees Celsius. Your results should be (in order and in Torr)

- Chemistry -
**DrBob222**, Sunday, February 26, 2012 at 7:56pmIt's hard to explain a number that doesn't show up in the writing. But I think the 40.67 is the heat vaporization of water although the problem lists it as 43.99.

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