**Problem Set #6 **

When possible, use the values for constants from our text. If you get them from other sources (if they are not in the book) cite where you got them from.

- (10 pts) The vapor pressure of Hg @ 20.00 °C is 1.201 millitorr. Calculate the vapor pressure of Hg dispersed as 65 nm droplets at this temperature. You may assume the density of Hg is 13.546 g/cm
^{3}. Surface tension in notes. - (20 pts) For the following solutions of components A and B, the following pressures were found. Xs are mol fractions in liquid, Ys are mol fractions in vapor.

X(A) | Y(A) | P (torr) |

0.0000 0.0490 0.3120 0.4750 0.6535 0.7905 1.0000 | 0.0000 0.0175 0.1090 0.1710 0.2550 0.3565 1.0000 | 255.6 257.9 211.3 184.4 156.0 125.7 55.03 |

Make 2 plots and use different colors for A and B. As a function of X(A), plot

- the Raoult’s law predictions (dashed lines), the P(A), P(B) and P curves, and the activities a(A) and a(B) based on Raoult’s law as the reference state.
- the activity coefficients, g(A) and g(B) based on Raoult’s law as the reference state.

3. (10 pts) for the following data for the partial pressure of Br_{2} dissolved in CCl_{4}, plot the data to determine the Henry’s law constant. Would you consider this an “ideal” system?

X(Br | P (torr) |

0 0.00394 0.00420 0.00599 0.0120 0.01300 0.02360 0.02380 0.02500 | 0 1.52 1.60 2.39 4.27 5.43 9.57 9.83 10.27 |

I didn’t ask for it here, but be sure you can calculate the activities and activity coefficients for H.L.