Given below is a set of Vapor Pressure (P) versus T (in K) data for a substance. Using the OWL graphing tool plot In(P) vs. 1/T (in x10³ units K-1) and determine the slope of the line. Vapor Pressure (kPa) T (K) 2.31 278 3.71 285 5.20 290 7.02 295 11.66 303 20.53 313 31.44 321 48.28 330 82.63 341

Consider the following data for the vapor pressure of diethyl ether, a widely used anesthetic in the early days of surgery. Follow the instructions in Question 13 to estimate the heat of vaporization of diethyl ether.

Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?

The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.