Using Henry's Law constants in Table 6.1 of Tinoco, calculate the solubility in M of each gas in water at 298 K if P(O2)= 0.2 bar, P(N2)= 0.75 bar, P(CO2)= 0.05 bar.

2. A and B form an ideal solution. At a total pressure of 0.90 bar, Xa(1)=0.65, XA(g) = 0.45. Using this information, calculate the vapor pressures of pure A and pure B.

The molar mass of liquid A = 85.0 g / mole, that of B = 112.0 g / mole. At 100 C, a solution of mass percentage in A equal to 30.0%, considered ideal, has a vapor pressureof equilibrium equal to 110 kPa. The vapor in equilibrium with this solution has a mole fraction of A equal to 0.450.(a) Determine the mass of A which must be added to 100 g of B to obtain a solution whosenormal boiling point is 100 C.   Please give the Answer

A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)

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