A polymer of large molar mass is dissolved in the organic solvent dimethylformamide (C3H7NO) at 25...
A polymer of large molar mass is dissolved in the organic
solvent dimethylformamide
(C3H7NO) at 25 °C, and the
resulting solution rises to a final height of 17.5
cm above the level of the pure solvent, as solvent molecules pass
through a semipermeable membrane into the solution. If the solution
contains 5.03 g polymer per liter, calculate the
molar mass of the polymer. Take the density of the solution to be
0.944 g cm-3.
Molar mass polymer =
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A polymer of large molar mass is dissolved in the organic
solvent dimethylformamide
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A polymer of large molar mass is dissolved in the organic solvent chloroform (CHCl3) at 25...
A polymer of large molar mass is dissolved in the organic solvent chloroform (CHCl3) at 25 °C, and the resulting solution rises to a final height of 7.99 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 3.97 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.48 g cm-3.
74 Percent Concentration -The amount of solute dissolved in a fixed amount of solvent is called the concentration of th...
74 Percent Concentration -The amount of solute dissolved in a fixed amount of solvent is called the concentration of the solution. Concentrations are typically expressed as Mass al.) (% m/m) which is the mass of the solute (g) divided by the mass of the solution [solute+ solvent] (g)x 1000/0; or as Volume ol.) (% v/v ) which is the volume of the solute in a fixed volume of solution (1O0mL of solution) x 1000/0; or less commonly in the laboratory,...
Polymer Chemistry: Problem 2. Polystyrene chains dissolved in cyclohexane at 35°C (theta conditions) can be separated...
Polymer Chemistry:
Problem 2. Polystyrene chains dissolved in cyclohexane at 35°C (theta conditions) can be separated by ultrafiltration according to molecular weight. The ultrafiltration process employs pressure-driven flow of a solution through a porous membrane to separate solutes by their molecular size. Molecules larger than the pore size are retained upstream of the membrane while smaller molecules pass through. In this exercise, the root mean square end-end- distance will be considered to provide an appropriate measure of molecular size. The...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kp=20.0....
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kp=20.0. 0.141 g of an unknown solute is dissolved in 7.90 g of cyclohexane (C6H12). The freezing point of the solution was 3.33ºC. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.132 g of the unknown is dissolved. The freezing point of the resulting solution was 0.75°C. Calculate the corresponding molar mass...
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved...
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...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a...
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypotheti...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
74 Percent Concentration -The amount of solute dissolved in a fixed amount of solvent is called the concentration of the solution. Concentrations are typically expressed as Mass al.) (% m/m) which is the mass of the solute (g) divided by the mass of the solution [solute+ solvent] (g)x 1000/0; or as Volume ol.) (% v/v ) which is the volume of the solute in a fixed volume of solution (1O0mL of solution) x 1000/0; or less commonly in the laboratory,...
Polymer Chemistry:
Problem 2. Polystyrene chains dissolved in cyclohexane at 35°C (theta conditions) can be separated by ultrafiltration according to molecular weight. The ultrafiltration process employs pressure-driven flow of a solution through a porous membrane to separate solutes by their molecular size. Molecules larger than the pore size are retained upstream of the membrane while smaller molecules pass through. In this exercise, the root mean square end-end- distance will be considered to provide an appropriate measure of molecular size. The...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kf=20.0. 0.147 g of an unknown solute is dissolved in 7.71 g of cyclohexane (C6H12). The freezing point of the solution was 3.38°C. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.139 g of the unknown is dissolved. The freezing point of the resulting solution was 0.85°C. Calculate the corresponding molar mass...
Molar Mass of a Solute The freezing point of cyclohexane is 6.50°C. For cyclohexane solvent Kp=20.0. 0.141 g of an unknown solute is dissolved in 7.90 g of cyclohexane (C6H12). The freezing point of the solution was 3.33ºC. Calculate the corresponding molar mass of the solute. g/mol 1homework pts Submit Answer Tries 0/5 To the above solution a further 0.132 g of the unknown is dissolved. The freezing point of the resulting solution was 0.75°C. Calculate the corresponding molar mass...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
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