3.(a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made bymixing CHCI3 and CH2C12 is ideal.i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25moles of components, what is the mass of CHCI3 present in that solution.

Given: Partial pressure of CHCl3 = 101 mmHg Partial pressure of CH2Cl2 = 235 mmHg Total pressure of…

(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume th mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmH moles of components, what is the mass of CHC13 present in

(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume th mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmH moles of components, what is the mass of CHC13 present in

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: A mixture of the vapors of two liquids A and B which form an ideal solution is contained within a…

A: The objective of the question is to calculate-The total pressure at condensationThe composition of…

Q: What is the vapor pressure above a mixture that is 40% (w/w) ethanol (CH3CH2OH) and 60% (w/w) water…

Q: The nonvolatile, nonelectrolyte cholesterol, C2-H460 (386.60 g/mol), is soluble in diethyl ether…

A: Osmotic pressure of solution is given as follows,

Q: e vapor pressure of a

Q: A (non-aqueous) solution is found to have a molality of 2.09 molal and experiences a freezing point…

A: Depression in freezing point is defined as the depression in freezing point of water on addition of…

Q: Toluene (C6H5CH3) and benzene (C6H₁) are two organic liquids with very similar properties, and when…

Q: Liquids A and B give ideal solutions. A vapor mixture which is 80% in mols of A is slowly compressed…

A: As per Dalton's law of partial pressure, the pressure exerted by a gas in the mixture of at least…

Q: skyscraper in Pittsburgh in the early 1970's is supported by water filled columns. Potassium…

A: Given that: Mass percent of K2CO3 = 40.0% Water is taking as solvent 40.0% by Mass K2CO3 means ,…

Q: The following is a T-x-y phase diagram for a binary system at constant pressure. a) Calculate the…

Q: Calculate the osmotic pressure in bar units glucose aqueous solution at 25.000C with a concentration…

A: Temperature = 25.00°C ...Or because °C + 273 = k ...So 25.00 °C + 273 = 298 k Concentration =…

Q: An antiseptic solution contains hydrogen peroxide, H2O2, in water. The solution is .5675 molal H2O2.…

A: The mole fraction of hydrogen peroxide is calculated in step 2.

Q: A 1.2 m aqueous solution of an ionic compound with the formula M2X3 has a boiling point of 102.8oC.…

A: The value for van't Hoff factor gets altered as per the compound's nature. It gets symbolized as…

Q: A solution is made by mixing 43.0 mL43.0 mL of ethanol, C2H6O,57.0 mL of water. Assuming ideal…

A: A solution is made by mixing 43ml of ethanol & 57mol of H2Owater vapor pressure of the two…

Q: A solution is prepared by dissolving 3.75 g of a non-volatile solute in 108.7 g of acetone and…

A: The objective of the question is to calculate the molar mass of a non-volatile solute that is…

Q: 3. a) The vapor pressure of water at 28 °C is 28.35 torr. Calculate the vapor pressure of at 28 °C…

Q: A 1 L solution is prepared by dissolving 200.0 g sucrose (C12H22O11; m.w. = 342.2965 g mol–1) in…

Q: A solution is made by mixing 46.0 mL46.0 mL of ethanol, C2H6O,C2⁢H6O, and 54.0 mL54.0 mL of water.…

Q: What is the molar mass of a non-electrolyte when 780 g of this compound is added to 3.0 kg of water…

A: Given that: Mass of non electrolyte (m’) = 780 g Mass of water (m”) = 3.0 Kg Change in boiling point…

Q: (+)-Carvone (C10H140) is a principal component of caraway and dill seed and is used as a food…

A: The calculation of molality requires the knowledge of moles of solute and mass of the solvent.…

Q: A gram of isprenoid was dissolved in 5 grams of camphor. he freezing point of the solution was…

Q: A (non-aqueous) solution is found to have a molality of 1.78 molal and experiences a freezing point…

A: Given :- molality of solution = 1.78 m Depression in freezing point (∆Tf) = 7.30 °C To calculate…

Q: The Henry's law constant for the solubility of nitrogen in water is 6.4 x 1o-4 M/atm at 25°C. At…

Q: 7) (+)-Carvone (C10H14O) is a principal component of caraway and dill seed and is used as a food…

A: We have carvone as C10H14O of mass 2.63g, in 14.6 ml of ethanol . We have to calculate the molality…

Q: 5 . If 40.2g NaCl are mixed into water and the total mass is 389g, what is the CHANGE in boiling if…

A: We have to calculate the change in boiling point , we have 40.2 g NaCl and 389 g of solution , Kb as…

Q: A solution is made by dissolving 44.5g of urea (H2NCONH2, a non-volatile non-electrolyte) in 260g of…

Q: 24. 100.0 grams of glucose (180.16 g mol-¹) is dissolved in 1000.0 grams of H₂O (18.02 g mol-¹).…

A: Given,mass of glucose = 100.0 gmolar mass of glucose = 180.16 g/molmass of H2O = 1000.0 gmolar mass…

Q: A solution that contains 3.86 g X in 150 g of ethyl acetate boils at 78.210C. What is the ,olecular…

A: Given: Mass of solute X = 3.86 g Mass of solvent ethyl acetate = 150 g The normal boiling point of…

Q: Determine the boiling point elevation of a solution of 110.0 mg of carvone (a.k.a. oil of spearmint,…

A: Given: The mass of carvone = 110.0 mg The mass of carbon disulfide = 1.40 g The molar mass of…

Q: What is the vapour pressure of a benzene-toluene solution at 30°C? State the answer in the form of…

A: Given data:Vapor pressure of pure benzene at 30 oC= 118 torrVapor pressure of pure toluene at 30 oC…

Q: Seawater contains about 3.5% by mass dis- solved solids. As a rough approximation, assume that the…

A: Well, in order to calculate the boiling point, we need to convert NaCl concentration in morality.…

Q: 70.0 grams of sugar (C12H22O11) is mixed with 465.0 mL of water. Calculate the molality and mole…

A: Molality can be defined as the number of moles of solute dissolved per kilogram of solvent. Solute…

Q: A 21.3 g sample of methyl alcohol (CH3OH) was dissolved in 24 g of water. The molar mass of CH3OH is…

Q: Equal masses of benzene (C6H6) and toluene (C7H8) are mixed together at 20 oC. If the vapor…

Question

3.
(a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane
(CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by
mixing CHCI3 and CH2C12 is ideal.
i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25
moles of components, what is the mass of CHCI3 present in that solution.

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

44. Calculate the molarity and molality of 268.3 mL of a solution containing 0.5142 mol of CsCl and 197.5 g of water. 52. Calculate the mole fraction of each component in a solution that is 15.7% by mass methyl alcohol, CH,OH, in water.
A solution is made by dissolving 45.0g of urea (H2NCONH2, a non-volatile non-electrolyte) in 312g of water. Calculate the vapour pressure of this solution at 25°C. (note the vapour pressure of pure water at 25°C is 23.8 torr.)
An antifreeze solution is prepared by mixing 1.00 L of water and 946 mL of ethylene glycol, C,H,O2 (molar mass = 62.07 g/mol). Calculate: (a) the mass percent of ethylene glycol in the mixture; (b) the mole fraction of ethylene glycol in the solution, and (c) the molality of ethylene glycol in the solution. (d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86°C/m; K = 0.512°C/m; density of EG = 1.114 g/mL)
A solution is made by dissolving 33.5g of urea (H₂NCONH₂, a non-volatile non-electrolyte) in 310g of water. Calculate the vapour pressure of this solution at 50°C. (note the vapour pressure of pure water at 50°C is 92.5 torr.)
The vapor pressure of pure ethanol (C2H5OH) at 60 °C is 0.459 atm. Raoults Law predicts that vapor pressure of a solution of 18.0 grams of glucose (C6H12O6, )not an electrolyte, non volatile) into 50.0 g of ethanol is....?
The partial pressure of O2 in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of O₂ can dissolve in 1.0 L of water at 25 °C if the partial pressure of O2 is 26 mm Hg? kí (O₂) = 1.3 × 10-³ Mass= g mol kg. bar
4. The vapor pressures of pure C5H12 and C6H14 at 298.15K are 511 torr and 150 torr, respectively. Determine the partial pressures of the components, and the composition (mole fractions) of the vapor above an equimolar mixture of these two liquids at 298.15K
both pls
A certain substance X condenses at a temperature of 111.6 C. But if a 200. g sample of X is prepared with 7.38 g of urea (NH2)2CO dissolved in it, the sample is found to have a condensation point of 111.9 C instead. Calculate the molal boiling point elevation constant Kb of X.
A (non-aqueous) solution is found to have a molality of 2.33 molal and experiences a freezing point depression of 4.00 degrees C. What is the Kf of the solvent (in degrees C/m)? HINT: Non-aqueous solutions do not tend to split into ions.