Use the Trouton's rule to estimate the normal enthalpy of vaporization of a material that boil at 147 oC and 1 atm. ΔvapH = __________ kJ/mol, 3 sig. fig. double check sign and unit.

Use Trouton's rule to estimate the enthalpy of vaporization for a substance whose boiling point is 80 C.

Determine the entrophy change of (kJ/K) associated to the conversion of 10 kg of ice at -11 degrees celcius to steam at 121 degrees celcius

Complete the following table. Calculate the vapor pressure, mm Hg, for each run. Vaporpressure, Pvapor = Pequil - Pinitial. Enter T and Pvapor from the preceding table in the following table. Complete the table by calculating the temperature in degrees Kelvin, the inverse of the temperature in degrees Kelvin, construct a graph of the natural logarithm of the measured vapor pressure,ln(Pvapor), versus1Twhere T is the average Kelvin temperature using the data from the four vapor pressure determinations.

Calculate the enthalpy of vaporization of acetamide given the following data table. Vapor Pressure (kPa) Temperature ("C) 1.000 102.8 10.000 150.8 100.000 218.2

The vapor pressure, P, of a certain liquid was measured at two temperatures, T. The data is shown in the table. ТК) Р (КРа) 225 3.40 725 7.58 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, AHvap, 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 = TOOLS x10 point 2: x = point 2: y = Determine the rise, run, and slope of the line formed by these points. rise = run = slope =

ANS B ONLY     a. The molar volume of a certain solid is 142.0 cm3 mol−1 at 1.00 atm and 427.15 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 152.6 cm3 mol−1.  At 1.2 MPa the melting temperature changes to 429.26 K. Calculate the enthalpy (KJ/mol) and entropy of fusion (J/mol-K) of the solid. b. Calculate the melting point of ice under a pressure of 10 MPa. Assume that the density of ice under these conditions is approximately 0.915 g cm−3 and that of liquid water is 0.998 g cm−3. From the result of the calculation, what happens when you increase the pressure on water, will it freeze or will the ice melt?