mmHg. You\'d like to mixture of 0.350 fraction ethanol 0.650 You have a li vapor

Question

mmHg. You'd like to mixture of 0.350 fraction ethanol 0.650 You have a li vapor formed at the calculate the bubble-point temperature of the mixture, and the composition of the bubble-point two ways. the first method, assume that the ideally and all components follow Raoult's law. What of the solution? Number What are the mole fractions of ethanol (e) and water (w) in the vapor phase at the bubble-point temperature? Number Number mol e mol mol w/ mol For the second method, use the Try diagram for the ethanol water system shown below. According to this diagram, what Vapor Liquid Equilibrium is the bubble-point temperature Mixture of Ethanol and Water of the 0.350 mol fraction 374 ethanol solution? (Note the 101.325 kPa requested units 372 Number 370 Previous GMe Alp Mew Solution Check Answer y Next Exit int

Explanation / Answer

1)

For ethanol:

A = 7.68117

B = 1332.04

C = 199.2

For water:

A = 8.07131

B = 1730.63

C = 233.426

P = 10 A – B / (C + T)

Partial pressure of ethanol, Pe = 0.35 * 10 A – B / (C + T)

Partial pressure of water, Pw = 0.65 * 10 A – B / (C + T)

Pe + Pw = PT = 760 mm Hg

Back calculating we get,

Tbp = 90.1 °C

Pe = 417.48 mm Hg

Pw = 342.52 mm Hg

Ye = Pe / PT

= 0.55

Yw = 1 – Ye = 0.45

2)

From the graph, for Xe = 0.35

Tbp = 355 K

= 355 – 273 °C = 82 °C

At 355 K

Ye = 0.6

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