Concept explainers
(a)
Interpretation:
The temperature of the mixture of benzene and toluene is to be calculated.
Concept introduction:
The formula to convert mass fraction
…… (1)
Here,
For two phase binary mixture, Raoult’s law states that,
…… (2)
Here,
Also, the partial pressure of the components in the two-phase binary system in terms of their vapor phase mole fraction is,
…… (3)
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
…… (4)
Here,
(b)
Interpretation:
The fraction of system’s mass present in the liquid phase is to be determined.
Concept introduction:
The formula to convert mass fraction
…… (1)
Here,
For two phase binary mixture, Raoult’s law states that,
…… (2)
Here,
Also, the partial pressure of the components in the two-phase binary system in terms of their vapor phase mole fraction is,
…… (3)
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
…… (4)
Here,
The formula to calculate density
…… (5)
The density of a mixture is calculated as:
…… (6)
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Chapter 6 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- The separation of aromatic compounds from paraffins is essential in producing many polyesters that are used in a variety of products. When aromatics and paraffins have the same number of carbon atoms, they often have similar vapor pressures, which makes them difficult to separate by distillation. Extraction is a viable alternative, as illustrated by the following simple system. Sulfolane (an industrial solvent) and octane may be considered completely immiscible. At 25°C, the ratio of the mass fraction of xylene in the octane-rich phase to the mass fraction of xylene in the sulfolanerich phase is 0.25. One hundred kg of pure sulfolane are added to 100 kg of a mixture containing 75 wt% octane and 25% xylene, andthe resulting systemis allowedto equilibrate. How much xylenetransferstothe sulfolane phase?arrow_forwardA water carbonating plant is available for use in the home and operates by providing carbon dioxide at 5.0 atm. Estimate the molal concentration, m (in mol/kg), of the soda water it produces. The Henry's law constant for CO2 in water at 25 °C is 1650 atm. Use the following representation of Henry' law: PB = xBKB where PB is the vapor pressure of the solute; xB is the mole fraction of the solute (mole per mole); and KB is the proportionality constant.arrow_forwardCalculate the following: (a) The bubble-point temperature of an equimolar mixture of liquid n-hexane and n-heptane at 1.0 atm and the composition (mole fractions) of the vapor in equilibrium with this mixture. (b) The dew-point temperature of a gas mixture with a molar composition of 30% n-hexane, 30% n-heptane, and 40% air at 1 atm and the composition (mole fractions) of the liquid in equilibrium with this mixture.arrow_forward
- 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.arrow_forwardb) Suppose you had a solution of 6.84 g of sugar (sucrose, C12HO1) in 90.0 g of water. (i) Calculate the number of moles of sugar and water present. (H=1; C=12; 0=16) (ii) Calculate the mole fraction of the water in the solution. (iii) At 100°C, the saturated vapour pressure of water at its boiling point is 101325 Pa. Calculate the vapour pressure of the solution at that temperature. (Remember to give your answer to a suitable number of significant figures.) (iv) Would the solution of sugar in water boil at this temperature, assuming the external pressure remains at 101325 Pa? Explain your answer.arrow_forwardThe 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?arrow_forward
- (A) It is required to separate 1 mole of ethanol from ethanol-water mixture by using distillation Column at standard conditions. After 1 hour, it is found that the volume was double and the pressure increased to 152 kpa. Find the Temperature after 1 hour by using the ideal gas law: PV = nRT Given : R = 0.082 L.atm/mole.K (B) Calculate the capacity of a Base added to a solution contains 10 mole of ammonia (k, = 1.8x105) and 6 mole of ammonium chloride in 120 ml? Note: Atomic weight: H = 1, 0 = 16, C = 12, Ba = 137, Cl= 35 , N=14arrow_forward(b) Surface sanitizers were prepared using ethyl alcohol/water and isopropyl alcohol/water solutions. An experiment was done to determine which composition would be most effective and as such two solutions were formulated: 70 % v/v ethyl alcohol and 70 % v/v isopropyl alcohol. Calculate the vapour pressure of these solutions and use your answer to reason which combination would stay on the surface longer. P° (Ethyl alcohol) = 12.4 kPa P° (Isopropyl alcohol) = 4.4 kPa P° (Water) = 2.4 kPaarrow_forwardThe partial molar volumes of water and ethanol in a solution with xH2O=0.45 at 25 ∘C are 17.0 and 57.0 cm3⋅mol−1, respectively. Calculate the volume change upon mixing sufficient ethanol with 4.30 mol of water to give this concentration. The densities of water and ethanol are 0.997 and 0.7893 g⋅cm−3, respectively, at this temperature. Express your answer to two significant figures and include the appropriate units.arrow_forward
- Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0.042 and 0.161. (i) Calculate the overall mole fraction of phenol in the mixture. (ii) Use the lever rule to determine the relative amounts of the two phases.arrow_forwardA mixture consisting of 1-mol-% ethane, 5-mol-% propane, 44-mol-% n-butane, and 50-mol-% isobutane is brought to a condition of 294.15 K (21°C) at pressure P. If the molar fraction of the system that is vapor is 0.2, what is pressure P (in bar), and what are the compositions of the vapor and liquid phases?arrow_forwardThe osmotic pressure of an aqueous solution at 300K is 250.0 kPa. (1)Calculate the molarity of solute (impurity) M (mol/m3)=[M]; (2) Calculate the molality of solute (impurity) b (mol/kg)=[b]; Calculate the freezing point of the solution T(oC)=[T]. Please pay attention to the sign. The cryoscopic constant Kf=1.86Kkgmol-1arrow_forward
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