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(c) Examine the detailed behavior of the UNILAN equation at zero pressure ( P -+0, n + 0)

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1436 In Ex 1410, Henry's constant for adsorption k, identified as the intercept on a plot of n/ P vs n, was found from a polynomial curve-fit of n/ P vs n An alternative procedure is based on a plot of In(P/n) vs n Suppose that the adsorbate equation of state is a power series inn: z = 1 + Bn + Cn2+ Show how from a plot (or a polynomial curve-fit) of ln(P/n) vs n one can extract values of k and B [Hint: Start with Eq (14105)] 1437 It was assumed in the development of Eq (14105) that the gas phase is ideal, with Z = 1 Suppose for a real gas phase that Z = Z ( T , P) Determine the analogous expression to Eq (14105) appropriate for a real (nonideal) gas phase [Hint: Start with Eq (14101)]

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1438 Use results reported in Ex 1410 to prepare plots of l vs n and z vs n for ethylene 7 adsorbed on a carbon molecular sieve Discuss the plots 1439 Suppose that the adsorbate equation of state is given by z = (1 - bn)-', where b is a constant Find the implied adsorption isotherm, and show under what conditions it reduces to the Langmuir isotherm 1440 Suppose that the adsorbate equation of state is given by z = 1+pn, where p is a function of T only Find the implied adsorption isotherm, and show under what conditions it reduces to the Langmuir isotherm 1441 Derive the result given in the third step of the procedure for predicting adsorption equilibria by ideal-adsorbed-solution theory at the end of Sec 148 1442 Consider a ternary system comprising solute species 1 and a mixed solvent (species 2 and 3) Assume that:

LOMBARDI RULE #2

Show that Henry's constant 'HI for species 1 in the mixed solvent is related to Henry's constants and for species 1 in the pure solvents by:

7 A To calculate the molality of a solution, both the moles of solute and the kilograms of solvent are needed A liter of solution would contain a known number of moles of solute To convert this liter to mass, a mass to volume relationship (density) is needed 8 E The mole fraction may be determined by dividing the vapor pressure of the desired substance by the sum of all the vapor pressures 87 mm Hg/(87 mm Hg + 170 mm Hg) = 034 9 C To produce a molar solution of any type, the final volume must be the desired volume This eliminates answers D and E B involves mass of water instead of volume A calculation of the required mass will allow a decision between A and B (30 L)(020 mol K3PO4/L)(212 g K3PO4/1 mol K3PO4) = 130 g K3PO4 10 C A 52 molal solution has 52 mol of methyl alcohol in one Kg (1000 g) of water The moles of water are needed (1000 g H2O)(1 mol H2O/180 g H2O) = 556 mol H2O The mole fraction may now be determined (52 mol CH3OH)/(52 + 556) mol = 0086 11 B The boiling point depends on the boilingpoint elevation (a colligative property) All colligative properties depend on the concentration of particles present C is a nonelectrolyte, thus, the concentration of the particles is 020 M All of the other substances are strong electrolytes The concentration of particles in each of these may be determined by multiplying the molarity given by the van t Hoff factor Each of these is calculated as follows: A: 2 010 = 020 D: 2 010 = 020 12 D (50 mole MgSO4/1000 mL)(1000 mL) (1204 g MgSO4/mol MgSO4) = 60 g MgSO4 B: 4 010 = 040 E: 2 010 = 020.

Here xi and xi are solute-free mole fractions:

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