The osmotic pressure values corresponding to 10 solutions of an enzyme in water at 298 K are given below. Using these values, calculate the molar mass ofthe enzyme? (Note: You can use the graph on the side for calculations.) c/(g dm) 1.00 2.00 4.00 7.00 9.00 ПРа 27.5 69.6 197 500 785 2 Mass concentration, 6 8 4 10 (up 6)ª5 Osmotic pressure, 100\r/G,MKP@lg dm)

The osmotic pressure values corresponding to 10 solutions of an enzyme in water at 298 K are given below. Using these values, calculate the molar mass ofthe enzyme? (Note: You can use the graph on the side for calculations.) c/(g dm) 1.00 2.00 4.00 7.00 9.00 ПРа 27.5 69.6 197 500 785 2 Mass concentration, 6 8 4 10 (up 6)ª5 Osmotic pressure, 100\r/G,MKP@lg dm)

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 128IP: Some nonelectrolyte solute (molar mass = 142 g/mol) was dissolved in 150. mL of a solvent (density =...

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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.
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?
The osmotic pressure of a solution of polystyrene in toluene (methylbenzene) was measured at 25 °C with the following results: c/(g dm− 3) 2.042 6.613 9.521 12.602 P/Pa 58.3 188.2 270.8 354.6 Determine the molar mass of the polymer. Molar Mass = __________ kg/mol.
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
The osmotic pressure of a solution of polystyrene in toluene (methylbenzene} was measured at 25 °C with the following results:c/(g dm-3) 2.042 6.613 9.521 12.602∏/Pa 58.3 188.2 270.8 354.6Determine the molar mass of the polymer.
Northern cod produce proteins that protect their cells from damage caused by subzero temperatures. Measurements of the osmotic pressure for two “antifreeze” proteins at 18°C yielded the data listed below. Use this information to calculate the molar mass for each of the proteins. Assume these proteins are nonelectrolytes and use the value i = 1. If a 53.7 mg sample of protein A in 1.5 mL of water has an osmotic pressure of 0.285 atm, what is the molar mass of protein A? If a 45.7 mg sample of protein B in 1.75 mL of water has an osmotic pressure of 0.218 atm, what is the molar mass of protein B?
You create an aqueous solution containing an unknown solute. Measuring the osmotic pressure, you find it is 0.2 bar. Which of the following data would you need in order to find the boiling temperature of the solvent at room temperature?a. The molecular weight of waterb. The mass of the solute in the solutionc. The ebullioscopic constant for water d. The cryoscopic constant for water e. No additional data is necessary.
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?
The molar mass of an enzyme was determined by dissolving it in water, and measuring the height, h, of the resulting solution drawn up a capillary tube at 20 °C. The following data were obtained.C/(mg cm-3) 3.221 4.618 5.112 6.722h/cm 5.746 8.238 9.119 11.990The osmotic pressure may be calculated from the height of the column, ∏= hpg, taking the mass density of the solution as p = 1.000 g cm-3 and the acceleration of free fall as g = 9.81 m s-2. Determine the molar mass of the enzyme.
Northern cod produce proteins that protect their cells from damage caused by subzero temperatures. Measurements of the osmotic pressure for two “antifreeze” proteins at 18°C yielded the data listed below. Use this information to calculate the molar mass for each of the proteins. Assume these proteins are nonelectrolytes and use the value i = 1. If a 57.9 mg sample of protein A in 1.5 mL of water has an osmotic pressure of 0.271 atm, what is the molar mass of protein A?
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In class, we derived the expression:ln XA =(ΔvH/R) ((1/T)-(1/T°))where A represents the solvent (and B would represent the solute, such that XA + XB = 1).Using the approximations given below, derive the expression:∆Tb = XB (RT°2/ΔvH)where ∆Tb is the change in boiling point between the solution and the pure liquid, T − T°.Approximations:ln(1 − X) ≈ −XTT° ≈ T°2Note: this derived expression is often simplified in General Chemistry as ∆Tb = Kbm where Kb is the boiling point elevation constant, and m is the molality.