on using the Clausius Clapeyron equation Find the vapor pressure of water at 29.7°C Express your answer to the tenths place. ___________ mm Hg
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on using the Clausius Clapeyron equation Find the vapor pressure of water at 29.7°C Express your...
Using the Clausius Clapeyron equation determine the vapor pressure of water at 50.0 degrees C. The molar heat of vaporization of water is 40.7 kJ/mol. How do you solve this?
8. (a) Use the Clausius-Clapeyron equation and calculate the vapor pressure (mm Hg) of butanone at 45 °C, given that the vapor pressure is 100 mm Hg at a temperature of 25 °C. The enthalpy of vaporization of butanone is 34.0 kJ/mol. (b) Calculate the enthalpy of vaporization for a compound if its vapor pressure is 26 mm Hg at 20°C and 167 mm Hg at 55 °C.
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)
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...
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
Use the Clausius-Clapeyron equation to calculate the temperature (°C) at which pure water would boil at a pressure of 400.0 torr. Temperature = ___°C the vapor pressure of h20 at this temperature is _____ torr.
Do sample problem 12.2. Use the Clausius-Clapeyron equation to solve this problem. At 34.1°C, the vapor pressure of water is 40.1 torr. What is the vapor pressure (in torr) at 84.1°C? The ΔHvap of water is 40.7 kJ/mol. Units need to match. R= 0.0821 l atm/mol K, R= 8.314 J/mol K. (12.1) (一) - - 号
1. (1.5 pts) Clausius Clapeyron. Show by calculation what is the vapor pressure of water at 45.0 °C. The normal boiling point of water is 100.0 °C and the heat of vaporization, AHap 40.7 kJ/mol. (Hint: you should know what P at the normal boiling point is.) 45.0 C
Determine enthalpy of vaporization graphically using the Clausius-Clapeyron equation. The vapor pressure of pentane (C5H12) has been measured over a range of temperatures. (a) Which of the following should give a linear plot (temperatures in K)? On the x-axis: — On the y-axis: C (b) When the appropriate plot is made, the resulting straight line has a slope of -3.38x103 K. Use this information to determine AHvap for C5H12. kJ/mol Check & Submit Answer Show Approach
Use of Clausius-Clapeyron Equation 3- The vapor pressure of liquid ethanol at various temperatures is given below. Estimate the heat of vaporization of this compound at 170. oW. Pbuh (kPa) 0.6667 1.333 2.667 5.333 8.00 13.33 T (°C)12.0-2.3 8.0 19.0 26.0 34.9 Equations P (RT/V-b))-(a/(T V(V+b))) (0.42748 R2 Tc25 ) / Pc b (0.08664 R Te ) / Pe a Use of Clausius-Clapeyron Equation 3- The vapor pressure of liquid ethanol at various temperatures is given below. Estimate the heat...