In this lab, you will determine the vapour pressure (P) of water at various temperatures and use this data to find its enthalpy of vaporization (AvapH). More generally, for an unknown liquid: if a plot of In P vs. 1/T gives a slope of -9260 K, what is its AvapH in kJ/mol? Do not worry about how realistic the value is. Assume R = 8.314 J mol-¹ K-¹. Answer:

In this lab, you will determine the vapour pressure (P) of water at various temperatures and use this data to find its enthalpy of vaporization (AvapH). More generally, for an unknown liquid: if a plot of In P vs. 1/T gives a slope of -9260 K, what is its AvapH in kJ/mol? Do not worry about how realistic the value is. Assume R = 8.314 J mol-¹ K-¹. Answer:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13ALQ

See similar textbooks

Similar questions

At 20.0 °C, the vapor pressure of ethanol is 5.95 kPa, and at 63.5 °C, its vapor pressure is 53.3 kPa. Use this information to estimate the enthalpy of vaporization for ethanol.
The normal boiling point of benzene is 80.1oC. What is the vapor pressure of benzene at 30.0oC? The ΔHvap of benzene is 30.7 kJ/mol
A mixture consists of 78,1 g benzene (C6H6) and 92,1 g toluene (C7H8). Both substancesare volatile, and their vapour pressures (in the pure form) are as follows at 20°C: Benzene: 0.0988 atmToluene: 0.0287 atm a) Which substance, benzene or toluene, would have the lowest boiling point in thepure form? Give a reason or your answer. b) Calculate the vapour pressure of the benzene-toluene mixture at 20°C.
A solution containing 1.470 g of dichlorobenzene in 50.00 g of benzene boils at 80.60 degree C and a pressureof 1.00 bar. The boiling point of pure benzene is 80.09 degree C, and the molar enthalpy of vaporization of purebenzene is 32.0 kJ/mol. Determine the molecular mass of dichlorobenzene
The standard enthalpy of vaporization of water, H2O, ΔvapH = 40.7 kJ/mol at 373 K. Assuming this value to remain constant at temperatures close to 373 K, use the Clausius-Clapeyron equation to estimate the vapor pressure of liquid water at 80°C.
The standard enthalpy of vaporization (H°vap) of ethylene glycol ((CH2OH)2) is 58.7 kJ/mol.The normal boiling point of ethylene glycol is 198.0°C.Calculate the vapour pressure of ethylene glycol at 164.5°C. (Units of pressure can be atm, torr, mmHg, Pa, kPa, bar, etc. -- units are always case sensitive)
Does the entropy of the system increase, decrease, or stay the same when a solid sublimes?
The normal boiling point of benzene is 80.1°C. What is its enthalpy of vaporization if the vapor pressure at 26.1°C is 100 torr?
SHOW COMPLETE SOLUTION AND WRITE LEGIBLY The normal boiling point of hexane is 69.0 °C. Estimate (i) its enthalpy of vaporization and (ii) its vapor pressure at 25 °C and at 60 °C. (Hint: Trouton’s rule).
The vapor pressure, ?,P, of a certain liquid was measured at two temperatures, ?.T. The data is shown in the table. T (K) P (kPa) 325 3.53 775 6.53 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, Δ?vap,ΔHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the ?x‑values and four significant figures in the ?y‑values. point 1: ?=x= point 1: ?=y= point 2: ?=x= point 2: ?=y= Determine the rise, run, and slope of the line formed by these points. rise=rise= run=run= slope=slope= What is the enthalpy of vaporization of this liquid?
In the study of the vapour pressure of chloroform is determined. Chloroform is placed in a container and allowed to reach a temperature op 28C. A vacuum is then created at which point the chloroform start to boil. The pressure and temperature are recorded. Subsequently the vacuum is gradually reduced by allowing a small amount of air into the vessel, thereby increasing the pressure in the vessel. At each of these higher pressures, the solution is heated and till it boils again and the temperature point and pressure is recorded at which the solution boils. This is repeated until the vessel reaches room pressure. What is the dependent and independent variable?
6. The normal boiling point of rhothanol is 70 °C. Given that the vapor pressure of rhothanol is 68.6 torr at 16.8 °C, calculate the molar enthalpy of vaporization of rhothanol.