Concept explainers
(a)
Interpretation:
The equations used to calculate the bubble-point temperature for the given mixture in the form
Concept introduction:
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
Here,
For two phase binary mixture, Raoult’s law states that,
Here,
(b)
Interpretation:
A spreadsheet is to be prepared to show the calculations by equations written in part (a). Also, test this spreadsheet for the given mixture at different pressures.
Concept introduction:
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
Here,
For two phase binary mixture, Raoult’s law states that,
Here,
(c)
Interpretation:
The spreadsheet prepared in part (b) is to be modified to incorporate the given Antoine equation and the bubble point temperature of the mixture is to be calculated at the given pressure.
Concept introduction:
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
Here,
For two phase binary mixture, Raoult’s law states that,
Here,
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Chapter 6 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solutionarrow_forwardCarbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/molarrow_forwardA solution is prepared by dissolving iodine, I2, in carbon tetrachloride, CCl4, at 25 °C. What is the mole fractions of the solute for a solute of molality 0.100 mol kg−1? (a) Mole fraction of solute = ________ 2 sig. fig. A solution is prepared by dissolving iodine, I2, in carbon tetrachloride , CCl4, at 25 °C. What is the mole fractions of the solvent for a solute of molality 0.100 mol kg−1? (b) Mole fraction of solvent = _____________. 3 sig. fig. A solution is prepared by dissolving iodine, I2, in carbon tetrachloride , CCl4, at 25 °C. For a solute of molality 0.100 mol kg−1, calculate the change in the chemical potential of the solvent caused by the solute. (c) change of chemical potential (solvent) = __________ J/mol. 3 sig. fig. R = 8.3145 J/Kmol.arrow_forward
- Estimate the molality (mol/kg) of oxygen in water at 25 °C and given that the partial pressure of O2 is 21 kPa near sea level (1 atm). (b) What would the solubility of oxygen be in water [O2] in (mmol/L)? (c) What is the solubility of [O2] in (mg/L) at that temperature? Henry’s constant for oxygen gas KO2 = 7.9 x 104 kPa kg mol-1.arrow_forwardOsmotic 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/mLarrow_forwardPlease indicate true (T) or false (F) as appropriate: Justify I) The vapor pressure of a solvent is reduced by the presence of a non-volatile solute II) In an ideal solution, the vapor pressure is increased by the presence of a solute Volatile. III) Sea water freezes at a lower temperature than sugar water. IV) In the laboratory, chemists use this effect to judge the purity of a component solid: if impurities are present, the freezing point of the compound is lower than the accepted value. A) TFTF B) TTFT C) FTFF D) TTTTarrow_forward
- 5) 50 g acetone (CH3COCH3) and 50 g methanol (CH;OH) are mixed to obtain a 100 g liquid solution at 25°C. Vapor pressures of acetone and methanol at 25°C are 271 mmHg and 143 mmHg, respectively. Assuming ideal mixing and evaporation behavior, calculate the followings: (a) Mole fractions of acetone and methanol in the solution. (b) Contribution of acetone and methanol to the total vapor pressure at 25°C. (c) The total vapor pressure at 25°C. (d) Composition of the vapor in terms of the mole fractions of acetone and methanol. (e) Given that the measured vapor pressure of this mixture is 161 mmHg, comment on your result in (d), what is the reason of the discrepancy? (CH3COCH3: 58 g/mol, CH;OH: 32 g/mol)arrow_forwardThe normal freezing point for para-dichlorobenzene (PDB) is 69.8oC. What will the freezing point be if 10.78 g of ethanol (CH3CH2OH) are dissolved in 40.0 g of PDB. (Kf = 7.10 oC*kg/mol, M.M.: CH3CH2OH = 46.068 g/mol, i = 1) solve and show stepsarrow_forwardConsider a solution containing two liquids A and B. In this mixture, the molar fraction of A is 0.3713. In addition, the partial molar volumes of A and B are worth 188.2 cm³ mol-1 and 176.14 cm³ mol-1 respectively. The molar masses of A and B are 241g mol-1 and 198g mol-1, respectively. At constant pressure and temperature, what is the volume of a solution of mass equal to 1kg? a - 1000 cm³ b - 843,5 cm³ c- 678,9 cm³ d - 364,3 cm³arrow_forward
- Fluorocarbons (compounds that contain both carbonand fluorine) were, until recently, used as refrigerants.The compounds listed in the following table are all gasesat 25 °C, and their solubilities in water at 25 °C and 1atm fluorocarbon pressure are given as mass percentages.(a) For each fluorocarbon, calculate the molality of a saturatedsolution. (b) Which molecular property best predictsthe solubility of these gases in water: molar mass,dipole moment, or ability to hydrogen-bond to water?(c) Infants born with severe respiratory problems are sometimesgiven liquid ventilation: They breathe a liquid thatcan dissolve more oxygen than air can hold. One of theseliquids is a fluorinated compound, CF3(CF2)7Br. The solubilityof oxygen in this liquid is 66 mL O2 per 100 mL liquid.In contrast, air is 21% oxygen by volume. Calculate themoles of O2 present in an infant’s lungs (volume: 15 mL)if the infant takes a full breath of air compared to takinga full “breath” of a saturated solution of O2 in…arrow_forwardThe following table presents the solubilities of severalgases in water at 25 °C under a total pressure of gas andwater vapor of 1 atm. (a) What volume of CH4(g) understandard conditions of temperature and pressure is containedin 4.0 L of a saturated solution at 25 °C? (b) Thesolubilities (in water) of the hydrocarbons are as follows:methane < ethane < ethylene. Is this because ethyleneis the most polar molecule? (c) What intermolecularinteractions can these hydrocarbons have with water?(d) Draw the Lewis dot structures for the three hydrocarbons.Which of these hydrocarbons possess p bonds?Based on their solubilities, would you say π bonds aremore or less polarizable than s bonds? (e) Explain whyNO is more soluble in water than either N2 or O2. (f) H2S is more water-soluble than almost all the other gasesin table. What intermolecular forces is H2S likely to havewith water? (g) SO2 is by far the most water-soluble gasin table. What intermolecular forces is SO2 likely to havewith…arrow_forwardST4D.3 - The vapor pressure of a substance at various mole fractions in a mixture were found to be as follows. Estimate the Henry's law constant [in MPa] for the substance for the particular solvent of this mixture. USE ALGEBRA instead of a graphical approach. Don't forget there's one more data point that isn't listed in the table (the origin). 0.00230.01020.0182 99.7 48.8 |P/КРа 27.7 Type your answer...arrow_forward
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