19.335 #2 N₁ und #5 02 sd 21.35 N1G) + 120297 M₂03 (5) initial ander temps 27.45°< Finglater tap 24.63% Calculate AHF Shen MASS OF GLORter 6000g SPOF GLORter 0.44) MASS OF LATER je 120009 SPrster N 4.18-1/8.5
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- K. C&H18 3 2 PPM1,324 A Calculate the masses of oxygen and nitrogen that are dissolved in 1.5 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. mass: FEB 22 ~ tv mg 0₂ MacBook Pro Henry's law constants for gases in water at 25 °C mass: Gas He N₂ 0₂ CO2 H₂S A O kh (bar - M-¹) 2.7 x 10³ 1.6 × 10³ 7.9 x 10² 29 10. W mgProve that M = (mole IL) %3D is % x 10 x d M. M.wt
- Calculate the masses of oxygen and nitrogen that are dissolved in 3.0 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. 0.55104 mass: Henry's law constants for gases in water at 25 °C Gas kn (bar-M-¹) He 2.7 x 10¹ N₂ 1.6 x 10' 0₂ 7.9 x 10² CO₂ 29 H₂S 10. 1.79 source: S, Rock, And Gallogly 46-General Chemistry | Publisher: University Books17. Match the following and choose the correct option. Column I Column II A. Molarity (M) Temperature р. B. Molality (m) q. Dilution C. Mole fraction (x) Volume г. D. Normality (N) Codes A C D (a) p, q, r q, r r 4, P (6) p, q, r q (c) 9, т (d) р, q р, 9, г р, т q, r p, qCalculate the solubility of nitrogen in water at an atmospheric pressure of 0.390 atm (a typical value at high altitude).Atmospheric Gas Mole Fraction kH mol/(L*atm)N2 7.81 x 10-1 6.70 x 10-4O2 2.10 x 10-1 1.30 x 10-3Ar 9.34 x 10-3 1.40 x 10-3CO2 3.33 x 10-4 3.50 x 10-2CH4 2.00 x 10-6 1.40 x 10-3H2 5.00 x 10-7 7.80 x 10-4
- 3. What is the mole fraction of methanol, CH;OH, (molar mass = 32.0 g/mol) in an aqueous solution that is 40.0% methanol by mass? (molar mass for H20 = 18.0 g/mol). %3D %3D А. 0.273 В. О.544 С. 0.101 D. 0.123 E. 0.315Osmotic 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- 2022.pdf - Adobe Acrobat Pro DC (32-bit) ndow Help oter 14 - Soluti. x 2 / 3 100% 9) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf=1.86°C/m. 9) A) -0.82°C B) -3.0°С С) -3.6°C D) -11°C 10) A solution of an 22.4 g of an unknown protein dissolved in enough water to make 0.150 L of solution has an osmotic pressure of 658 torr at 25°C. Based on these data, what is the molar mass of the protein? 10) search hp
- Consider the solution process below. Select the true statement. AH1 AH, AH Expanded solvent Expanded solute Solute Solvent Step 1 Step 2 AH3 Direct formation of solution Step 3 AH3 is endothermic. O Enthalpy of solutions, AHsolution = AH1 + AH2 + AH3 %3D The greater the intermolecular force between solute molecules, the more exothermic AH, is. O AHsolution is always positive.If a 0.890 m aqueous solution freezes at -2.10 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i =(D) A sample of gas at 1.08 atm and 25°C has a SO₂ concentration of 1.55 µg/m³ and is in equilibrium with water. The Henry's Law constant for SO2 in water is 2.00 M atm¹ at 25°C. Ideal gas volume = 22.4 dm³ at 1 atm pressure and 0°C. i) Calculate the SO₂ concentration in the sample in ppm. ii) Calculate the SO2 concentration in water at 25°C. (