Calculate the vapor pressure of ethanol, CH3CH₂OH, in a water solution containing 82.5% ethanol by volume at 19.0 °C. The vapor pressure of pure ethanol at 19.0 °C is 40.0 Torr. The density of ethanol is 0.789 g.mL-¹ and the density of water is 1.000 g.mL-1.

Calculate the vapor pressure of ethanol, CH3CH₂OH, in a water solution containing 82.5% ethanol by volume at 19.0 °C. The vapor pressure of pure ethanol at 19.0 °C is 40.0 Torr. The density of ethanol is 0.789 g.mL-¹ and the density of water is 1.000 g.mL-1.

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

Related questions

Q: Calculate the molality of chloride ions in an aqueous solution of magnesium chloride in which the…

A: To solve this problem we will use the formula of molality

Q: Calculate the molality of chloride ions in an aqueous solution of magnesium chloride in which the…

Q: K,= 2.57 °C kg mol for a certain subs 20 colution freezes at 5.7 °C. Calculate the freezing point of…

A: At freezing point of liquid there exists equilibrium between solid particles and solvent phase.…

Q: The normal freezing point of a certain liquid X is -2.7 °C, but when 12.2 g of urea ((NH,),CO) are…

Q: A certain liquid X has a normal freezing point of 6.90°C and a freezing point depression constant…

A: The freezing point of a solution made of 92.g of glycine (C2H5NO2) dissolved in 700. g of X is 2.93…

Q: A certain liquid X has a normal freezing point of 3.00°C and a freezing point depression constant…

A: Given : Mass of solute i.e benzamide, C7H7NO = 80.7 g Mass of solvent i.e X = 900 g = 0.900 Kg…

Q: Calculate the molality of alum and the molality of the cream of tartar in the solution of mordant.…

A: Given: mass of Alum = 2 g mass of cream of tartar = 1 g Volume of water = 100 mL molar mass of Alum…

Q: Calculate the molality of 35.0 grams of KBr dissolved in 450.0 mL pure water.

Q: A 24.7% solution of HCl by mass has a density of 1.12g/cm^3. Calculate the molarity of HCl in the…

A: A 24.7% solution of HCl by mass has a density of 1.12g/cm^3. We have to calculate the molarity of…

Q: The freezing point of acetic acid is 17.0 °C, and its Kf is 3.90 °C·kg/mol. If dissolving an amount…

A: In this question, we want to determine the moles of solute in the Solution. You can see details…

Q: 1. The solubility of L-glutamic acid (an amino acid) in water has been determined to be as follows…

A: Solubility: When the maximum amount of solute is dissolve in the solvent is called solubility. On…

Q: A certain liquid X has a normal boiling point of 114.40 °C and a boiling point elevation constant K…

A: The boiling point of the pure liquid = 114.40 0C. The boiling point of the solution = 115.1 0C.…

Q: Calculate the vapor pressure (in torr) at 25 °C of a solution containing 49.8 mL ethylene glycol…

A: EWe know ,Ps = P0Xsolvent

Q: What is the solubility of argon (in units of grams per liter) in water at 25 °C, when the Ar gas…

Q: What would be the freezing point, in degree Celsius, of 3.8 m aqueous solution of Sc(ClO 4 )3? k f…

A: Molality of solution (m) = 3.8m Freezing point (Kf) = 1.86 C/m Freezing point (T) = ?

Q: 10.0 g of an organic substance is dissolved in 80.0 g of benzene. The freezing point of the solution…

A: Mass of benzene = 80.0 g = 0.080 Kg mass of organic solute = 10.0 g Freezing point of this solution=…

Q: A solution was made by mixing 6.25 g of heptane (C7H63, molar mass = 100.21 g/mol) with 46.2 g of…

Q: When you open a bottle of a carbonated beverage, bubbles of carbon dioxide gas escape from the…

A: Henry’s Law:Henry's Law explains the solubility of gas in a liquid solution. It states that the…

Q: The molal freezing point depression constant K,=2.51 °C·kg•mol -1 for a certain substance X. When…

A: Given that: Mass of urea = 6.12 g Mass of X = 100.g Kf of X solvent = 2.51°C.kgmol-1 Freezing…

Q: Antifreeze is composed mainly of ethylene glycol (C2H6O2, d = 1.11 g/cm3). It is added to a car…

A: The relationship between depression in freezing point (∆Tf) and molality of solition is ∆f = kf ×…

Q: At 20 °C, the concentration of dissolved oxygen in water exposed to gaseous oxygen at a partial…

A: Since you have asked multiple question, we will solve the first question for you as per our…

Q: The freezing point of a liquid will change when a solute is added. Explain how the addition of salt…

A: When a solute is dissolved in the water, the vapor pressure of the solution is lower than the pure…

Q: The addition of salt to water decreases the chemical potential of the water.

A: The statement is True. The decrease in chemical potential occurs because the concentration of water…

Q: The vapor pressure of water at 30 °C is 4.24 kPa. Calculate the vapor pressure if 95.0 g of…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: Formula used Xsolvent = Psolution/ Psolvent where Xsolvent = mole fraction of solvent Psolution…

Q: A certain liquid X' has a normal freezing point of -3.40 °C and a freezing point depression constant…

A: The question is based on the concept of depression in freezing point. on adding solute to a…

Q: The common laboratory solvent ethanol is often used to purify substances dissolved in it. The vapor…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: When a solute is added in pure solvent then its vapor pressures gets lowered. It is referred as a…

Q: An aqueous solution is 20.0% by mass of sodium thiosulfate pentahydrate, Na, S2 O3-5H2O. What is the…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves…

A: Since you have posted multiple questions, we will provide the solution only to the first five…

Q: Ice cubes from a freezer have a temperature of about -12°C (10°F), which is cold enough, but contact…

A: Det Tf=i ×Kf×m ion ,i for Nacl-->Na+ +Cl- i=2

Q: the solute mentioned. Increasing the temperature of a solution of a salt that has an enthalpy…

A: Here we have to explain the factors that increase or decrease the solubility of solute in solvent at…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: Formula used Xsolvent = Psolution/ Psolvent where Xsolvent = mole fraction of solvent Psolution…

Q: At 20.0∘C, the concentration of dissolved oxygen in water exposed to gaseous oxygen at a partial…

Q: At 25 °C, the solubility of NaCl is 36.0g/100g H20. How much NaCl can dissolve in 450 g of water at…

A: The solubility of the solution is determined by the maximum amount of solute dissolved in the given…

Q: A 0.547 g sample of an unknown solute dissolved in 14.0 g of tert-butanol produces a solution with a…

A: At a specific temperature, when vapor pressure of any particular substance in its liquid and solid…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: Raoult's law states that the relative lowering in vapour pressure of an ideal solution containing…

Q: The vapor pressure of an aqueous solution of copper(II) sulfate at 38 °C is 0.06430 atm. The vapor…

Q: A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant…

A: We have to predict the freezing point of solution.

Q: What is the mole fraction of acetone, C3H6O, in the vapor phase from a solution consisting of a…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: #Q.1: Given the vapor pressure of pure diethyl ether, Po = 463.57 mm Hg Moles of aspirin added =…

Q: The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte…

A: Since you have asked multiple question, we will solve the first question for you as per our…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Solutions of hydrogen in palladium may be formed by exposing Pd metal to H₂ gas. The concentration of hydrogen in the palladium depends on the pressure of H₂ gas applied, but in a more complex fashion than can be described by Henry's law. Under certain conditions, 0.56 g of hydrogen gas is dissolved in 197 g of palladium metal. (The density of the resulting solution is 11.7 g/cm³.) (a) Determine the molarity of this solution.
5. The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in benzene is TNT. Calculate the vapor pressure of the solution at 25 °C when 12.12 grams of TNT, C,H;N;Os (227.1 g/mol), are dissolved in 155.7 grams of benzene. benzene = CHs = 78.12 g/mol.
The freezing point of acetic acid is 17.0 °C, and its Kf is 3.90 °C·kg/mol. If dissolving an amount of solute into 4.862 g of acetic acid results in a solution having a freezing point of 15.9 °C, how many moles of solute are in the solution?
What is the mole fraction of propanol, CH3CH2CH2OH, in the vapor phase from a solution consisting of a mixture of propanol and isopropanol, (CH3)2CHOH, at 25.00 °C, if the total pressure above the solution is 35.29 torr? The vapor pressures of pure propanol and NaN at 25.00 °C are 20.90 torr and 45.20 torr, respectively.
The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.Calculate the vapor pressure of the solution at 25 °C when 10.18 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 239.0 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.VP(solution) = mm Hg
A solution is prepared by adding 0.108 moles of Mg(NO3)2 to 1.00 mole of water. Calculate the vapor pressure of this solution at 55 °C.The vapor pressure of pure water at 55 °C is 118.1 Torr. Assume that the Mg(NO3)2 is completely dissociated. 365 Torr 28.9 Torr 89.2 Torr 107 Torr 97.1 Torr
10. Consider 18.32 g benzoic acid that is dissolved in 1.00 kg benzene (CeHe). The resulting solution has a freezing point depression of 0.384°C. Given that K(C6H6) 5.12°C kg.mol-¹: (a) Calculate the molar mass (g.mol-¹) of one "solute" particle in solution without looking up the chemical formula for benzoic acid.
Consider a body of water in equilibrium with solid calcium sulfate, CaSO4, for which Ksp = 3.0 * 10^-5 at 35 degrees C. Calculate the solubility, in g/L of calcium sulfate in water assuming that other reactions are negligible.
A certain liquid X has a normal freezing point of 7.00°C and a freezing point depression constant =Kf 7.41·°C·kgmol−1. A solution is prepared by dissolving some iron(III) chloride (FeCl3) in 700.g of X. This solution freezes at 3.5°C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.
The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,
Calculate the vapor pressure of ethanol, CH₃CH₂OH, in a water solution containing 72.5% ethanol by volume at 19.0 °C. The vapor pressure of pure ethanol at 19.0 °C is 40.0 Torr. The density of ethanol is 0.789 g·mL⁻¹ and the density of water is 1.000 g·mL⁻¹.