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1) The molar heat of vaporization of a hydrocarbon is 5360 calories. The vapor pressure at...
Given the vapor pressure of water at 60 C is 149.3 mmHg, find the molar heat of vaporization of water.
From the following vapor pressure data for butanol, an estimate of the molar heat of vaporization of C,H,OH is kJ/mol sted P, mm Hg T, Kelvins 40.0 326 100 343
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.
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}
Revised 6/22/17 Station # Date me- - -- CHM 112 Vapor Pressure and Heat of Vaporization Pre-Lab Questions Solve the Following Problem: Using the Clausius- Claypeyron Equation to Determine the Heat of Vaporization from Experimental Measurements of Vapor Pressure. The Vapor Pressure of Dichloromethane was measured as a function of Temperature, and the following results were obtained: Vapor Pressure (mmHg) 0.8 Temperature (K) 200 220 240 260 280 300 97 391 Determine the Heat of Vaporization of Dichloromethane. Use an...
The vapor pressure of water at 25C is 23.8 mmHg. The average heat of vaporization between 25 and 40C is about 10,400 cal/mol. Using Clausius-Clapeyrone equation, calculate the vapor pressure at 40C? Equation used: log(p2/p1) = (ΔH*ΔT)/(2.303*R*T1*T2) Answer: 55.2 mmHg Just need a worked out solution to see what I'm doing wrong.
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.
Vapor pressure measurements at several different temperatures are shown for mercury. Determine graphically the molar heat of vaporization for mercury.
1)2)1)The vapor pressure of ethanol is \(1.00 \times 10^{2} \mathrm{mmHg}\) at \(34.90^{\circ} \mathrm{C}\). What is its vapor pressure at \(63.16^{\circ} \mathrm{C}\) ? ( \(\mathrm{AH}_{\text {vap }}\) for ethanol is \(39.3 \mathrm{~kJ} /\) mol. )\(\mathrm{mmHg}\)2)Calculate the amount of energy (in kJ) necessary to convert \(457 \mathrm{~g}\) of liquid water from \(0^{\circ} \mathrm{C}\) to water vapor at \(187^{\circ} \mathrm{C}\). The molar heat of vaporization \(\boldsymbol{H}_{\mathrm{vap}}\) ) of water is \(40.79 \mathrm{~kJ} / \mathrm{mol}\). The specific heat for water is \(4.184 \mathrm{~J} /...