2) Draw the isobaric phase diagram at 1 atm of the following two-component liquid system: water (Boiling point = 100°C) and nitric acid (Boiling point = 86°C), with the mass percentage of nitric acid on the x-axis. When the liquid mixture contains 68 % nitric acid, an azeotrope with a boiling point of 120.5°C, is formed. Use the sketch to describe under which conditions pure nitric acid can be obtained by means of isobaric distillation.
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- The 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 CH41g2 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 6 ethane 6 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 p 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 water?Toluene (C6H5CH3) and benzene (C6H₁) are two organic liquids with very similar properties, and when they are mixed, they form an ideal solution. A mixture contains 35,6 g of toluene and 125 g of benzene. Toluene has a vapour pressure of 22 mm Hg, and benzene has a vapour pressure of 75 mm Hg at 25°C. (a) Which compound, toluene or benzene, would have the highest boiling point? Motivate your answer. Calculate the total vapour pressure over the mixture at 25°C. (b)At 90°C, the vapor pressure of methylbenzene is 53.3 kPa and that of 1,2-dimethylbenzene is 20.0 kPa. What is the composition of a liquid mixture that boils at 90°C when the pressure is 0.50 atm? What is the composition of the vapor produced?
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- Cyclohexanol (C6H12O) has a cryoscopic constant of 42.2 K kg mol−1, an Ebullioscopic constant of 3.5 K kg mol−1, a freezing point of 25.93 ∘C, and a boiling point of 161.8 ∘C. Anna dissolves 20.00 g of naphthalene (C10H14) into 200.0 mL of cyclohexanol (d = 0.962 g mL−1). What is the freezing point and boiling point of the solution?A gaseous mixture of two substances under a total pressure of 0.8 atm is in equilibrium with an ideal liquid solution. The mole fraction of substance A is 0.5 in the vapor phase and 0.2 in the liquid phase. What are the vapor pressures of the two pure liquids? Pls answer thank you so muchOsmotic 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
- 3. The vapour pressure of water at 50.0°C is 92.50 torr. When 12.6 g of glycerol are dissolved in 494 g of water, the vapour pressure is lowered to 92.04 torr. (a) What is the molar mass of glycerol? (b) What is the molecular formula of glycerol (a compound containing C, H, and O) from the following combustion analysis: when 2.00 g glycerol are combusted, 2.865 g CO₂ and 1.564 g H₂O are recovered.1. Ideal solution composition of A and B liquids at 80°C is 100 (for A) and 600 (for B) mmHg, respectively. (a) Construct the P-x phase diagram by calculating the compositions of the liquid and vapor phases. (b) 1.0 mole of solution with ZB= 0.60 at 80°C is in an open container and is evaporated until the total vapor pressure decreases by 20%. Calculate the number of moles of the liquid and vapor phases using the leverage rule.3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane (CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25 moles of components, what is the mass of CHCI3 present in that solution.