The enthalpy of vaporization of acetone is 32.0kJ/mol. The normal boiling point of acetone is 56.5 degrees Celcius. What is the vapor pressure of acetone at 25 degrees Celcius?
Ok I think I need to use the Clausius-Clapeyron equation:
but then I only have 4 out of the 6 unknowns, delta H, T2, T1 and R. If this is the correct method, then how do I find P1?
Ok I think I need to use the Clausius-Clapeyron equation:
but then I only have 4 out of the 6 unknowns, delta H, T2, T1 and R. If this is the correct method, then how do I find P1?
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"The normal boiling point of acetone is 56.5 degrees Celcius."
At this point, the vapor pressure equals the ambient pressure.In this case, normal indicates 1 atm of pressure. So, at 56.5 C, the vapor pressure of the acetone is 760 mmHg (or 1.00 atm or 101.325 kPa, whichever set of pressure units you are using).
At this point, the vapor pressure equals the ambient pressure.In this case, normal indicates 1 atm of pressure. So, at 56.5 C, the vapor pressure of the acetone is 760 mmHg (or 1.00 atm or 101.325 kPa, whichever set of pressure units you are using).
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Think about the definition of NORMAL boiling point -- It is the saturation temperature at 1 atm pressure.