4 The osmotic pressure of a protein solution wasmeasured at 25°C. The following data wereobtained.c (g dm-3)2.0426.6139.52112.602П (Ра)58.3188.2270.8354.5Use this data to determine the molar mass of theenzyme in g mol-1.

Answered: Image /qna-images/answer/d9b649b3-7ae7-4be4-be8f-f786c4d7b50b.jpg

Answered: The osmotic pressure of a protein…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 129QRT

See similar textbooks

Similar questions

Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density = 0.879 g/cm3). The elevated boiling point of the solution was 355.4 K. What mass of solute was dissolved in the solvent? For the solvent, the enthalpy of vaporization is 33.90 kJ/mol, the entropy of vaporization is 95.95 J/K mol, and the boiling-point elevation constant is 2.5 K kg/mol.
The solubility of ethylene (C2H4) in water at 20 C and 0.300 atm pressure is 1.27 104 molal. (a) Calculate the Henrys law constant for this gas in units of molal/torr. (b) How many grams of ethylene are dissolved in 1.00 kg water at 20 C if the pressure of the gas is 500 torr?
Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/mol
Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solution
Yeasts are able to produce high internal concentrations of glycerol to counteract the osmotic pressure of the surrounding media. Suppose that a sample of yeast cells were placed in a 4% sodium chloride solution by weight. Density of solution at 25 °C = 1.02 g/mL MW of solute = 58.44 g/mol i of glycerol = 1 R = 0.08205 L-atm/mol-K At the same temperature, what will be the molar concentration of glycerol considering the computed osmotic pressure of the solution and the normal osmotic pressure inside a yeast cell of 7.3 atmospheres?
Calculate the osmotic pressure in bar units glucose aqueous solution at 25.000C with a concentration of 0.15 mol L-1.
The molality of an aqueous solution of sugar (C12H22O11) is 2.58 m. Calculate the mole fractions of sugar and water.
you dissolve 1.0g of the enzyme in water to make 250mL of solution. You measure the osmotic pressure and find it to be 3.5Torr at 298K. what is the molar mass of the enzyme?
A solution containing 56 mg of a protein in 30 mL ofdistilled water exerts an osmotic pressure of 0.01 atmat T 5 258C. Determine the molecular weight of theunknown protein
The boiling point of an aqueous solution containing sucrose (C12H22011) is 101.45\deg C. Calculate the osmoticpressure of this solution at 39\deg C, at which the solution density is 1.036 g/mL.
A solution is prepared by dissolving 20.0mg of insulin in water and diluting to a volume of 5.00mL gives an osmotic pressure of 12.5 mm Hg at 300K. What is the molecular weight of insulin?
Suppose that a solution made from an unknown solute dissolved in solvent X. Its molality is 0.0125 and it boils 0.047oC higher than solvent X's boiling point. With the use of valid approximations, calculate the osmotic pressure of the said solution at 60oC? The following are useful thermodynamic data for solvent X to solve the problem: ΔSvap=87.92 J*K-1mol-1 Tb=61.15oC density at 60oC=1.394 g/cm3

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

The osmotic pressure of a protein solution was measured at 25°C. The following data were obtained. c (g dm-3) 2.042 6.613 9.521 12.602 П (Ра) 58.3 188.2 270.8 354.5 Use this data to determine the molar mass of the enzyme in g mol-1.