When ethanol is added to water at 25 °C and 1 bar, the total volume of the solution changesaccording to the empirical functioncmx - 0.36394cm(mol EtOH)= **V = 1002.93 cm + 56.6664mol EtOHcm(mol EtOH)+ 0.028256-where x is the number of moles of ethanol in the solution.As ethanol is added to the solution, the partial molar volume of ethanol decreases, reaches aminimum, and then increases. This behavior is shown in the figure below.Find the function for (ma) find the value x = ng56Ong TPHow many moles of ethanol are present when the partial molarvolume of ethanol in the solution is minimum?How many moles of water are present if the mole fraction ofethanol with this amount of ethanol present is 0.0952?535.*- nmol10Is the partial molar volume of water increasing, decreasing with increasing x, at a maximum orat a minimum? Explain based on an equation based on an equation from the lecture slides.Partial melar volume, VAcm mot

A mole is defined as some of the chemical units it may be atoms, molecules, ions.…

Answered: When ethanol is added to water at 25 °C…

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

Thirty milliliters of ferrous ammonium sulfate solution contain 1.176 grams of pure FeSO4·(NH4)2SO4·6 H2O.Twenty milliliters of potassium dichromate solution contain 0.2940 gram of K2Cr2O7 Calculate the normality of potassium dichromate solution
An aqueous solution of mass of 100 g of aqueous copper II sulfate CuSO4.xH₂O was prepared by dissolving aqueous copper II sulfate in 54 g of water. If the mole fraction of CuSO4 was known to be 0.05 Calculate the value of x?
Given: Mass of lauric acid (g): 8.000g Mass of benzoic acid (g): 1.027g Freezing temperature of pure lactic acid(°C): 43.3°C Freezing point of the benzoic acid-lauric acid mixture(°C): 39.8°C Question: Calculate molality (m,) in mol/kg, using the formula ΔTf = m × Kf. The Kf value for lauric acid is 3.9°C x kg/mol.
A student determined the molar mass of an unknown ionic solid by the method used in this experiment. She found the equilibrium temperature of the ice water mixture (THE FREEZING POINT) to be 0.50°C on her thermometer. When she added 3.10 g of her solid to the mixture, the temperature fell to -4.30°C. She then poured off the solution into a beaker. The mass of the solution was 34.59 g. Kf = 1.86°C/m What was the freezing point depression ∆Tf (celsius) What was the molality of the unknown solution? How much water was in the solution? What did she find to be the observed molar mass of the ionic solid, assuming she made the calculation properly?
#31 & 32
It is desired to prepare 2.5 m^3 of a 60 mol percent methanol - water solution. Determine the volumes of methanol and water required to be mixed at ambient temperature given that the partial molar volumes of methanol and water are 58.3x10^-6m^3/mol and 17.2 x 10 m^3/mol respectively. The density of the methanol is 782.51 kg/m^3. Do not use chatgpt. Thank you!
The graph given below plots the (approximate) partial molar volumes of ethanol (black line) and water (red line) in units of ml/mole at 25°C in a mixture as a function of the mole fraction of ethanol. Use the information in this graph (note the different y axes for water and ethanol) and the densities at 25°C to calculate the resulting total volume of the g following two mixtures.(pethanol = 0.789 ml & PH20 = 0.998 ) ml a. 150 ml ethanol + 100 ml H2O b. 200 ml ethanol + 40 ml H2O H20 VELOH Vet o*HA -V ELOH V H2O T 0.8 1.0 0.2 0.4 0.6 0.0 XELOH 53 54 55 57 15 18
Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
Calculate freezing temperature Tf and the boiling temperature Tb of a solution formed by mixing 15.6g of magnesium chloride, strong electrolyte with 155g of acetic acid, freezing point in 17.0 Celsius and boiling point of 118 Celsius. the Kf and Kb for the solvent are 3.90 Celsius/m and 3.07 Clesius/m respectively Explain in a paragraph your reasoning of your answer
At 25 °C the solubility of lead(Il) bromide is 2.70 x 10 mol/L. Calculate the value of Kgp at this temperature. Enter your answer in exponential format using a capital "E (example 1.23E-4) and no units (value 2%).
Based on the following data, determine the molecular weight of the unknown solute. Note the "initial freezing point" refers to the freezing point of the solvent as a pure substance while the "final freezing point" refers to the freezing point of the mixture. Mass Solvent: 15.000 g FPD Constant of Solvent: 4.9 Mass Solute 2.350 g Initial Freezing Point: 85.3oC Final Freezing Point: 82.4oC Your answer should follow the format: a) ΔT b) Molality of the Solution c) mols of solute d) Molecular weight of Solute
A semi-permeable membrane separates the contents of cell. The concentration of sodium ions is 2.1 L.atm mol mol K.mol outside of the cell and 2.5 inside of the cell. The ideal gas constant R= 8.206 x 10 -2 L L and room temperature is about 20°C or 293 K. (a) Determine the osmotic pressure (in atm) and the tonicity of the solution surrounding a cell with radius of 0.013 mm at room temperature. П= (b) The solution surrounding the cell is O Hypotonic O Hypertonic O Isotonic atm

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS