Answer the last question V. RESULTSIn Excel (or another spreadsheet), tabulate the vapour pressure and temperature data collected during theexperiment. You should only input your last measurement at room temperature (Le when all of the air was out of theisoteniscope). The other pressure readings taken at this temperature are inaccurate since the acetone vapour in theisoteniscope was contaminated with air. In subsequent columns, calculate In P,T (in Kelvin) and 1/T (K').Plot In Pas a function of 1/T. This plot is not expected to be a perfectly straight line. However, curvature is notalways detectable at the precision of our temperature and pressure measurements. Therefore, we will assume linearityand that the value of AH, that will eventually be obtained is a good one for the midpoint of the In P vs. 1/T data. Obtainthe slope of the best-fit line by a regression analysis and add the line to your graph. In order to calculate the enthalpyof vaporization at the midpoint we must have an accurate value of the compressibility factor, Z, for acetone at thetemperature and pressure of the midpoint.To deduce Z certain additional information is necessary. If only two terms are used the virial equation reduces toZ =1+Bin which V is the molar volume and B is the second virial coefficient. The best values of B are those below in Table 1,which were given to us by Dr. Peter Golding. A small interpolation may be needed to obtain Z precisely at your midpointtemperature, or you could simply use the value at 310 K. Calculate P at your midpoint temperature (or 310 K) usingthe equation for In P:In P = a +B/TNow, modify the virial equation by eliminating V, using V =. obtaining a quadratic equation in Z. Introduce P.T and B at the midpoint (or 310 K) and solve for Z. Be sure to use proper units, preferably Sl units. Notice that B isgiven in units of cm mol- (or ml. mol-).Finally, calculate the enthalpy of vaporization from the slope of your fit for the midpoint (or 310 K) and report itsvalue, in J mol-L. Also, since we assume that conditions are reversible, or nearly so, and that AH, is consequentlyequivalent to q,a. you may calculate the entropy of vaporization, AS, at the same temperature. 1/T (K^-1)IIn(p)0.00345.2840.003350.003295.515.7360.003245.9346.12In(p)0.003196.26.165.95.85.75.65.55.45.35.2123456

Vaporization is the process of transitioning of the liquid state of a substance into its vapor…

Finally, calculate the enthalpy of vaporization from the slope of your fit for the midpoint (or 310 K) and report its value, in ] mol-¹. Also, since we assume that conditions are reversible, or nearly so, and that A/, is consequently equivalent to qr you may calculate the entropy of vaporization, AS,, at the same temperature.

Finally, calculate the enthalpy of vaporization from the slope of your fit for the midpoint (or 310 K) and report its value, in ] mol-¹. Also, since we assume that conditions are reversible, or nearly so, and that A/, is consequently equivalent to qr you may calculate the entropy of vaporization, AS,, at the same temperature.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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