From the following vapor pressure data for butanol, an estimate of the molar heat of vaporization...
From the following vapor pressure data for diethyl ether, an estimate of the molar heat of vaporization of C2H5OC2H5 isP, mm Hg T, Kelvins40.0 245100 262Express the answer in terms of kJ/mol.Please show work so I can understand.
1) The vapor pressure of liquid antimony is 400 mm Hg at 1.84×103 K. Assuming that its molar heat of vaporization is constant at 115 kJ/mol, the vapor pressure of liquid Sb is _____ mm Hg at a temperature of 1.81×103 K. 2) The normal boiling point of liquid acetone is 329 K. Assuming that its molar heat of vaporization is constant at 29.0 kJ/mol, the boiling point of CH3COCH3 when the external pressure is 1.21 atm is ______ K.
The vapor pressure of liquid antimony is 400 mm Hg at 1.84x10' K. Assuming that its molar heat of vaporization is constant at 115 kJ/mol, the vapor pressure of liquid Sb is m m Hg at a temperature of 1.81x10' K.
Given the heat of vaporization of benzene as 30.8 kJ/mol and the vapor pressure = 92 mm Hg at 25°C. Calculate the vapor pressure of benzene at 75°C.
The vapor pressure of substance X is 100. mm Hg at 1080.°C. The vapor pressure of substance X increases to 600. mm Hg at 1220.°C. Determine the molar heat of vaporization of substance X using the derived form of the Clausius-Clapeyron equation given below. (Include the sign of the value in your answer.) ____ kJ/mol
A liquid has a vapor pressure of 150 torr at 60ºC. The molar heat of vaporization for this substance is 40.8 kJ/mol. Determine the normal boiling point of this liquid. {ln(P1/P2 ) = ∆Hvap/R(T1-T2/T1T2) = ∆Hvap/R(1/T2 - 1/T1); ln P = 2.303 log P}
Use the References to access important values if needed for this question. The vapor pressure of liquid butanol, C4H9OH, is 40.0 mm Hg at 326 K. A sample of C4H9OH is placed in a closed, evacuated container of constant volume at a temperature of 462 K. It is found that all of the C4H9OH is in the vapor phase and that the pressure is 54.0 mm Hg. If the temperature in the container is reduced to 326 K, which of...
Water has a vapor pressure of 23.8 mm Hg at 25°C and a heat of vaporization of 40.657 kJ/mol. Using the Clausius-Clapeyron equation given below, determine the vapor pressure of water at 96°C. ln P2 P1 = −ΔHvap R 1 T2 − 1 T1 _______________ mm Hg (pay attention to sig figs)
A. Vapor Pressure Measurements Vapor Pressure (mm Hg) *53.5 3.51 623 4.41 Temp.(°C) Temp.(K) Gol 219.3 11.0 292.2 23.2 296.4 26.0 30112 _ 1/T 00368 .00342 .60331 60332 .00323 - 4.61 lib. 214.2 4.75 5.367 36.0 309.2 Sample Calculations: Oct 213,15=k 6.1 +218,15 = 214,3 279300368 k' Use your data above to prepare an Excel or LoggerPro graph of In P vs. 1/T. Have Excel or LoggerPro draw the best fit straight line through the data points and determine the...
15. According to the Clausius-Clapeyron equation ln va R T T P"арф) refers to the vapor pressure at temperature 1, R-2 cal/mol-K, and Ah is the heat of changc associated with the process of transitioning to the vapor (cither sublimation or vaporization depending on whether the transition is from solid to vapor or liquid to vapor) i.e., дН-H vapor-H , where X is either solid or liquid and H denotes the corresponding molar enthalpy. Use the Clausius-Clapeyron equation to solve...