1. (1.5 pts) Clausius Clapeyron. Show by calculation what is the vapor pressure of water at...
Suppose the boiling point of pure water at high altitude is 88.46 °C. Use the Clausius-Clapeyron equation to determine the atmospheric pressure (atm) at this high altitude. The normal boiling point of water is 100.0 °C at 1 atm, and its heat of vaporization is 40.7 kJ/mol.
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?
Use the Clausius-Clapeyron equation to predict the boiling point of water at 8.4 atm. The boiling point of water at 1.00 atm is 100 °C, the heat of vaporization of water is ΔHvap=40.660 kJ/mol. Enter your result, without the unit, in °C, to a precision of 0.1 °C
Use the Clausius-Clapeyron equation to predict the boiling point of water at 8.4 atm. The boiling point of water at 1.00 atm is 100 °C, the heat of vaporization of water is ΔHvap=40.660 kJ/mol. Enter your result, without the unit, in °C, to a precision of 0.1 °C.
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.
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
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...
i need help with this page. please be organized. thank you - () - C, D) Activity: Clausius-Clapeyron Equation The Clausius Clapeyron equation allows us to find the vapor pressure at one temperature if we know the vapor pressure at another temperature and the AH Use the Clausius-Claperyon equation (given below) to solve the following problem. 1. Methanol has a normal boiling point of 64.6°C and a heat of vaporization (AHp) of 35.2 kJ/mol. What is the vapor pressure of...
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...