Compound EZ has a molar mass of 76.10 g/mol.A Calculate the solute mole fraction and molality of an aqueous solution that is 15% EZ by mass. The molar mas of water is 18.02 g/mol.Your answer.mole fraction of EZmolality:B. At 40 °C, water has a vapor pressure of 55.3 torr. What is the vapor pressure of the solution described in item A at 40 °C assuming EZ is a non-volatile non electrolyte.molalYour answertorrC.if in his case compound EZ is 70% dissociated into E" and Z, deterrfine the freezing point of the solution described in item A. For water, K, = 1.86 °C/m.Your answer"CSUBMIT YOUR SOLUTIONS ON THE NEXT PAGE.

Molar mass of EZ = 76.10 g/mol Concentration of solution = 15% by mass Molar mass of water = 18.02…

Compound EZ has a molar mass of 76.10 g/mol. A. Calculate the solute mole fraction and molality of an aqueous solution that is 15% EZ by mass. The molar mass of water ia 18.02 g/mol. Your answer. mole fraction of EZ molality molal B. At 40 C, water has a vapor pressure of 55.3 tor. What is the vapor pressure of the solution described in itern A at 40 °C assuming EZ is a non-volatile non-electrolyte. Your answer torr Cin this case compound EZ is 70% dissociated into E and z, deterine the freezing point of the solution described in item A. For water, K= 1.86 "C/m

Compound EZ has a molar mass of 76.10 g/mol. A. Calculate the solute mole fraction and molality of an aqueous solution that is 15% EZ by mass. The molar mass of water ia 18.02 g/mol. Your answer. mole fraction of EZ molality molal B. At 40 C, water has a vapor pressure of 55.3 tor. What is the vapor pressure of the solution described in itern A at 40 °C assuming EZ is a non-volatile non-electrolyte. Your answer torr Cin this case compound EZ is 70% dissociated into E and z, deterine the freezing point of the solution described in item A. For water, K= 1.86 "C/m

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 54E: At a certain temperature, the vapor pressure of pure benzene (C6H6) is 0.930 atm. A solution was...

See similar textbooks

Similar questions

Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the salt concentration is high and swell when the salt concentration is low. In a 25C aqueous solution of NaCl, whose freezing point is 0.406C, erythrocytes neither swell nor shrink. If we want to calculate the osmotic pressure of the solution inside the erythrocytes under these conditions, what do we need to assume? Why? Estimate how good (or poor) of an assumption this is. Make this assumption and calculate the osmotic pressure of the solution inside the erythrocytes.
Calculate the freezing point and normal boiling points of each of the following aqueous solutions. (a) 2.63 m acetic acid (b) 33.0 % by mass lactose, C12H22O11 (c) 32.15 mL of ethylene glycol, C2H6O2(d=1.113g/mL) in 624 mL of water (d=1.00g/mL)
A 12-oz (355-mL) Pepsi contains 38.9 mg caffeine (molar mass = 194.2 g/mol). Assume that the Pepsi, mainly water, has a density of 1.01 g/mL. For such a Pepsi, calculate: (a) its caffeine concentration in ppm; (b) its molarity of caffeine; and (c) the molality of caffeine.
An aqueous solution contains 0.180 g of an unknown, nonionic solute in 50.0 g of water. The solution freezes at 0.040 C. What is the molar mass of the solute?