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
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Use the Clausius-Clapeyron equation to predict the boiling point of water at 8.4 atm. The boiling...
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.
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.
Determine the AHvap in kJ/mol using Clausius-Clapeyron equation given that the boiling at 1.5 atm of a substance is 400 K, and its normal boiling point is 348 K. (Only enter numericanswer to its first decimal place, do not enter unit kJ/mol) P2 In P1 -AH/1 R T2 "G. =)
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
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?
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
I know that I have to use the clausius clapeyron equation, but I
think I am getting lost in the algebra. So please include the full
algebra. Thanks!
Here are the answers:
9. Consider the following water and planetary data: Earth Surface temperature: 20 °C Earth surface pressure: 1 atm Boiling point of water on Earth: 100 °C Mars surface temperature: -50 °C Mars surface pressure: 0.015 atm Freezing point of water on Mars: 0 °C a. What is the...
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)
The clausius-clapeyron equation relates the temperature and
the pressure of a chemical system to it's Heat of
vaporization.
fure and the pressure of a chemical system 2. The Clausius-Clapeyron Equation relates the temperature and the pres to its Heat of Vaporization (AH...): P. AH (1 1 ) re and pressure of a system, from which the mined. Below is a table of data for one of Experiments are conducted to measure the temperature and pressure Heat of Vaporization (AH..) for...