The vapor pressures of the components, A and B, in a binary solution have been modeled and found to obey PA = XAPA* exp(XB²) PB = XBPB* exp (X₁²) where XA and XB are the mole fractions, and PA* and PB* are the vapor pressures of each pure substance. (a) If PA* = 0.175 bar and PB* = 0.126 bar, compute the total vapor pressure (in bars) of the mixture when XB = 0.68. (b) Assuming that the vapor is an ideal gas, what are the mole fractions of each component in the vapor phase?

The graph given below plots the (approximate) partial molar volumes of ethanol (black line) and water (red line) in units of ml/mole at 25°C in a mixture as a function of the mole fraction of ethanol. Use the information in this graph (note the different y axes for water and ethanol) and the densities at 25°C to calculate the resulting total volume of the g following two mixtures.(pethanol = 0.789 ml & PH20 = 0.998 ) ml a. 150 ml ethanol + 100 ml H2O b. 200 ml ethanol + 40 ml H2O H20 VELOH Vet o*HA -V ELOH V H2O T 0.8 1.0 0.2 0.4 0.6 0.0 XELOH 53 54 55 57 15 18

we are calculating the molar mass from the freezing point depression. What would the effect be on calculated molar mass if the thermometer was not properly calibrated andconsistently reads 1.3oC too high?

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