A 1.137 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9Cl3 Og). When the sample is dissolved in water to a total volume of 34.9 mL, the osmotic pressure of the solution is 3.86 atm at 299 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: x10 TOOLS % %

A 1.137 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9Cl3 Og). When the sample is dissolved in water to a total volume of 34.9 mL, the osmotic pressure of the solution is 3.86 atm at 299 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: x10 TOOLS % %

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A solution is made from 540.0 g sucrose (C₁₂H₂₂O₁₁, MM = 342.3 g/mol) dissolved in water to a total volume of 551 mL of solution at a temperature of 52.0 °C. Calculate the osmotic pressure of solution. R = 0.08206 L･atm/K･mol
A 0.751-g sample of protein is dissolved in 50.0 mL of solution, and the solution exhibits an osmotic pressure of 4.1 torr at 25oC. Calculate the molar mass of protein. (R = 0.08206 L.atm/(mol.K); 1 atm = 760 torr; assume the protein is nonelectrolyte)
The nonvolatile, nonelectrolyte aspirin, C9Hg 04 (180.10 g/mol), is soluble in diethyl ether CH3CH₂OCH₂CH3. Calculate the osmotic pressure generated when 11.5 grams of aspirin are dissolved in 207 ml of a diethyl ether solution at 298 K. The molarity of the solution is The osmotic pressure of the solution is M. atmospheres.
When 2.60 g of a nonelectrolyte solute is dissolved in water to make 275 mL of solution at 29 °C, the solution exerts an osmotic pressure of 915 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? mol moles of solute: What is the molar mass of the solute? molar mass: g/mol
The nonvolatile, nonelectrolyte estrogen (estradiol), C18H24O2 (272.4 g/mol), is soluble in chloroform, CHCl3.Calculate the osmotic pressure generated when 14.5 grams of estrogen are dissolved in 240. ml of a chloroform solution at 298 K.The molarity of the solution is _______.The osmotic pressure of the solution is ______ atmospheres.
2⁰ A 1.212 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9Cl3Og). When the sample is dissolved in water to a total volume of 34.2 mL, the osmotic pressure of the solution is 4.15 atm at 297 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: % %
The nonvolatile, nonelectrolyte DDT , C14H9C15 (354.5 g/mol), is soluble in diethyl ether CH;CH,0CH,CH3. How many grams of DDT are needed to generate an osmotic pressure of 3.10 atm when dissolved in 298 ml of a diethyl ether solution at 298 K. grams DDT
In a laboratory experiment, students synthesized a new compound and found that when 14.61 grams of the compound were dissolved to make 210.0 mL of a ethanol solution, the osmotic pressure generated was 1.91 atm at 298 K. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? Molar mass = g/mol
A 1.384 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9C13Og). When the sample is dissolved in water to a total volume of 41.2 mL, the osmotic pressure of the solution is 3.83 atm at 305 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: % %
When 3.25 g of a nonelectrolyte solute is dissolved in water to make 165 mL of solution at 24 °C, the solution exerts an osmotic pressure of 879 torr.What is the molar concentration of the solution? MHow many moles of solute are in the solution? molWhat is the molar mass of the solute? g/mol
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 °C. What is the average molar mass of starch? (Becausenot all starch molecules are identical, the result will be an average.) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
The osmotic pressure (in atm) of 0.499 M K2SO4 solution at 298 K is ______? Give your answer to three sig figs.