Lecture_5b

# Lecture_5b

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Unformatted text preview: n the limit of an infinitesimal change in the number of moles of water. Mathematically, we write V W =,Lim0 DV = dV . n W @ Dn W dn W Once we impose the conditions that temperature, pressure and the number of moles of ethanol, nE, are to be held constant, the derivative on the right hand side becomes identical to the definition of the partial molar volumes used above and in Eq. (5.33): V W = æ ¹V ö ç ¹n ÷ è W ø T , P, n E An example of the applications of Eq. (5.33): Consider a 40% by mass ethanol solution of ethanol in water at 25°C. From the figure of partial molar volumes of ethanol and water in the presence of each other, estimate the volume of 1000 g of the solution. Compare this to the volume that would have resulted if the solution was ideal. Density of ethanol = 0.785 g mL–1 and pure water = 0.997 g mL–1 , at this temperature. In 1000 g of solution, we have 400 g ethanol (E) and 600 g water (W). 400 g nE = = 8.68 mol. 46.07 g mol −1 600 g nW = = 33.30 mol. 18.02 g mol −1...
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## This document was uploaded on 02/28/2014 for the course CHEM 311 at LA Tech.

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