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The osmotic pressure of an unknown, nonelectrolytic compound dissolved in 2.3L of solution is 8.31 atm...
The osmotic pressure of a solution containing 2.04 g of an unknown compound dissolved in 175.0 mLof solution at 25 ∘C is 2.13 atm . The combustion of 22.08 g of the unknown compound produced 36.26 g CO2 and 14.85 g H2O. What is the molecular formula of the compound (which contains only carbon, hydrogen, and oxygen)?
0.35g of an unknown compound dissolved in 100.0ml of water ahas an osmotic pressure of 32.6 mmhg at 15C. calculate the molar mass of the compound, answer 2 3 sig figs
100. mL of solution and is found to have an osmotic pressure of 28.1 mmHg at 20°C. Calculate the molar mass of the compound. (1 atm 760 mmHg) 1 0.102 g of an unknown non electrolyte solute is dissolved in enough water to make A. 663 g/mol B. 0.872 g/mol C. 1.15 g/mol D. 727 g/mol E. 1.10 x 102 g/mol
0.0140 grams of Cr(NH3)sCls was dissolved in 25.00 mL of water to give an osmotic pressure of 128.28 mmHg at 298.0 K. How many ions were produced per molecule? Note: R - 0.0806 L atm/mol K, MM Cr(NHs)Clh 243.5 g/mol alculate the osmotic pressure as if Cr(NH3)sCls did not ionize then use the relationship t: C true vapor pressure nonionized vapor pressure
5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 mL of solution. The osmotic pressure at 25C is 278.0 torr. What is the molar mass of the solid? 6a. Calculate the van't Hoff factor of a 0.085M potassium sulfate solution that has an osmotic pressure of 5.4atm at 25C 5. 1.024 g of an unknown molecular solid are dissolved in enough water to produce 200.0 ml. of solution. The osmotic pressure at 25...
XXIII. An isotonic solution will produce an osmotic pressure of 7.84 atm measured against pure water at human temperature (37.0 °C). How many grams of sodium chloride must be dissolved in 500 mL of water to produce an isotopic solution? Na = 23.00; CI = 35.45 A) 9.01 g B) 4.51 g C) 18.0 g D) none of them
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...
6. A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor. The resulting solution melted at 176.0 C. What is the molecular mass of the compound? The melting point of pure camphor is 179.5 C. The freezing-point-depression constant for camphor Kf is 40.0 C/m. 7. A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at...
I’m just missing these two questions ? Help please P24. What is the osmotic pressure π), in atm, at 25 °C of an aqueous solution containing 2.75 grams of beryllium fluoride, BeF2, dissolved in 500 mL of water? BeF2 is an electrolyte compound. [Hint: van't Hoff Factor] & (R 0.0821 L atm/mol K) 2.61 atm b) 3.05 atm 7.15 atm 8.59 atm
. 0.275 L of solution is prepared by dissolving 2.50 g of an unknown molecular compound in enough water. The osmotic pressure of this solution is 1.98 atm at 27 °C. (R = 0.08206 L·atm/mol·K) a) Determine the molar mass of the molecular compound. (7 pts) b) If you need to prepare 0.275 L of AlCl3 solution with the same osmotic pressure of the above solution, what mass of AlCl3 (MW = 133.33 g/mol) would you need to weigh out?