The vapor pressure of acetone (C3H,O) at 39.5°C is 400 torr. (a) If the boiling point of acetone is 56.5°C, calculate its enthalpy of vaporization (AH,vap; in kJ/mol). (b) Using calculated (AH,vap and vapor pressure at 39.5, calculate the vapor pressure of acetone at 25°C. (R = 8.314 J/(mol.K))

(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).

ow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Use the References to access important values if needed for this question. Liquid propanol (C3H¬OH) has a normal boiling point of 97.2 °C and liquid pentanol (C;H|OH) has a normal boiling point of 138 °C. (a) In which of the two are the intermolecular forces the weakest? (b) Which of the two would you expect to have the highest viscosity at 25 °C? | Submit Answer Try Another Version 1 item attempt remaining ot pt Previous Cengage Learning | Cengage Technical Support 888 & %23 24 7 8 3. 4 R T. Y K D C V

The vapor pressure of ethanol (C2H5OH) at 19 °C is 40.0torr. A 1.00-g sample of ethanol is placed in a 2.00 L containerat 19 °C. If the container is closed and the ethanolis allowed to reach equilibrium with its vapor, how manygrams of liquid ethanol remain?

Energy to sublime Na(s) = 109.0 kJ/molElectron affinity of Cl(g) = -349.0 kJ/molFirst ionization energy of Na(g) = 495.0 kJ/molBond energy of Cl2(g) = 240.0 kJ/molΔHrxn for Na(s) + 1/2 Cl2(g) → NaCl(s) = -411.2 kJ/mol   Determine the lattice energy of NaCl(s), using the data provided.

Toluene (C7H8) is a common laboratory solvent with ΔH°vap = 38.1 kJ/mol. If the vapor pressure of toluene at 89.6 °C is 380. torr, at what temperature, in °C, will toluene have a vapor pressure of 507 torr?

Ethanol, with ΔHvap = 40.5 kJ mol-1, has a higher ΔHvap than methanol, which is 35.2 kJ mol-1, due to its larger size and greater intermolecular forces. Because the ΔHvap for ethanol is larger, we would expect that for the two liquids to reach the same vapor pressure, the temperature for ethanol would have to be higher. If the vapor pressure is 0.0992 atm at 27.3 °C, what would the temperature be when the vapor pressure is 4.52 atm?

19. The 50:50 (by mass) mix of water and ethylene glycol (antifreeze) contains 16 moles of ethylene glycol per 1 kg of water. Given than K₁ for water is 0.5 °C/m, what is the boiling point of the mixture? (A) 92 °C (B) 99.5 °C (C) 100 °C (D) 100.5 °C (E) 108 °C

What is Δq for the vaporization of 50.0 g of Compound A (76.03 g/mol;  ΔHvap is 31.6 kJ/mol)?