The following relation describes the volume change in a water (solvent – species 1) and salt (solute – species 2) solution: V=1.001+16.625n2 +56.092 n23/2 +119.4n22 where V is expressed in units of liters, and n2 in kmole. (1) Obtain an expression for partial V2 in terms of n2, and determine partial V2 when x2 is approching 0 in liter per kmole. (2) Obtain an expression for partial V1 one in terms of n2, and one in terms of x1.

The sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 1.09g as a gas, calculate the pressure in the can when it is stored at 25 0C.  (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093M

Refer to the ternary phase diagram in Fig. 5E.4. How many phases are present, and what are their compositions and relative abundances, in a mixture that contains 2.3 g of water, 9.2 g of trichloromethane, and 3.1 g of ethanoic acid? Describe what happens when (i) water, (ii) ethanoic acid is added to the mixture.

Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL

Aniline, C6H5NH2, and hexane, C6H14, form partially miscible liquid–liquid mixtures at temperatures below 69.1 °C. When 42.8 g of aniline and 75.2 g of hexane are mixed together at a temperature of 67.5 °C, two separate liquid phases are formed, with mole fractions of aniline of 0.308 and 0.618. (i) Determine the overall mole fraction of aniline in the mixture. (ii) Use the lever rule to determine the relative amounts of the two phases.

The partial molar volumes of water and ethanol in a solution with H₂O = 0.45 at 25 °C are 17.0 and 57.0 cm³ mol-¹, respectively. -1 Part A AV = Calculate the volume change upon mixing sufficient ethanol with 8.20 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g cm 5, respectively, at this temperature. Express your answer to two significant figures and include the appropriate units. Submit μÅ Value Request Answer Units Review | Constants I Periodic Table . ?

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) A where ΧΑ 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 XB = 0.68. (b) Assuming that the vapor is an ideal gas, what are the mole fractions of each component in the vapor phase?

At 39.9 ◦C, a mixture of ethanol (x1 = 0.9060, p1 = 130.4 Torr) and isooctane ( p2 = 43.9 Torr) forms a vapor phase with molar fraction y1 = 0.6667 at a total pressure of 185.9 Torr. (a) Calculate the activity and activity coefficient of each component. (b) Calculate the total vapor pressure that the mixture would have if it were ideal.

Dibromoethene (DE, p*DE = 22.9 kPa at 358 K) and dibromopropene (DP, p*DP = 17.1 kPa at 358 K) form a nearly ideal solution. If zDE = 0.60, what is (a) ptotal when the system is all liquid, (b) the composition of the vapour when the system is still almost all liquid.

There is a 15.85% by mass aqueous KCl (molecular weight 74.5513 g mol–1) solution at 25 °C. The density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Could you please find osmotic pressure?