Fle| CAsersluser/Desictop/CHT002%20-620Cepy/Tutorial-Man 20CH1002 pdf O Maps t 18 Q D Page view A ad aioud V Draw Y Highight Q fras 3. The vapour pressure of water at 25°C is 23.8 mm Hg. What is the vapour pressure of a solution containing 5.50 grams of non-electrolyte sucrose (molar mass = 342 g/mole) in 12.8 g of water (molar mass-18.0 g/mole) at 25 °C?

Fle| CAsersluser/Desictop/CHT002%20-620Cepy/Tutorial-Man 20CH1002 pdf O Maps t 18 Q D Page view A ad aioud V Draw Y Highight Q fras 3. The vapour pressure of water at 25°C is 23.8 mm Hg. What is the vapour pressure of a solution containing 5.50 grams of non-electrolyte sucrose (molar mass = 342 g/mole) in 12.8 g of water (molar mass-18.0 g/mole) 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

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 =...

See similar textbooks

Similar questions

1 At a temperature of 302.8 K, mixtures of phenol andwater exist as two separate phases with mole fractionsof phenol of 0.30 and 0.93. Use the lever rule to determine the relative amounts of the two phases for amixture w ith an overall mole fraction of phenol of 0.45.
Determine the molar solubility (in mol/dm3) of solute A in a binary mixture at 1.32 bar if Henry’s constant is 3.80x102 KPa kg mol-1. The density of A is 0.95 kg dm-3
A solution containing 30 g of non-volatile solute exactly in 90 g of water has a vapour pressure of 2.8 kPa at 298 K. Further 18 g of water is added to this solution. The new vapour pressure becomes 2.9 kPa at 298 K. Calculate:(i) the molecular mass of solute and(ii) vapour pressure of water at 298 K.
The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?
Two substances A and B are known to form ideal liquid solutions. A vapour mixture containing50% (mol) A and 50% (mol) B is at 311 K and 101.3 kPa. This mixture is compressedisothermally until condensation occurs. At what pressure does condensation occur and what isthe composition of the liquid that forms? The vapour pressures of A and B are 142 kPa and 122kPa respectively.
Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0. 0 42 and 0 .161 . (a) Calculate the overall mole fraction of phenol in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases .
At 25 °C, the vapour pressure of pure benzene is 12.8 kPa and the vapour pressure of pure methylbenzene (toluene) is 3.8 kPa. Consider a liquid mixture with mole ratio 30% benzene-70% methylbenzene, which you can treat as an ideal liquid mixture, in a closed container. a) Calculate the mole ratio of benzene and methylbenzene in the vapour.
At 300 K, the vapour pressures of dilute solutions of HCI in liquid GeCI4 are as follows: x(HCI) 0.005 0.012 0.019p/kPa 320 76.9 121 .8 Show that the solution obeys Henry's law in th is range of mole fractions and calculate Henry's law constant at 300 K.
Consider the following solutions at 20 °C:I: 0.5 moles trifluoroacetic acid in 1.0 mole of waterII: 0.5 moles trifluoroacetic acid in 1.0 mole of acetonitrileWhich solution would have the greater vapour pressure? Justify your answerfully with calculations
Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0.042 and 0.161. (i) Calculate the overall mole fraction of phenol in the mixture. (ii) Use the lever rule to determine the relative amounts of the two phases.
The following temperature-composition data were obtained for a mixture of octane (O) and methylbenzene (M) at 1.00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapour at equilibrium. The boiling points are 110.6oC and 125.6oC for M and O, respectively Plot the temperature-composition diagram for the mixture. What is the composition of the vapour in equilibrium with the liquid of composition (i)Xm =0.250 and (ii) Xo =0.250?
Comelli and Francesconi examined mixtures of propionic acid with various other organic liquids at 313.15 K (F. Comelli and R. Francesconi, J. Chem. Eng. Data 41, 101 (1996)). They report the excess volume of mixing propionic acid with tetrahydropyran (THP, oxane) as VE = x1x2{a0 + a1(x1 − x2)}, where x1 is the mole fraction of propionic acid, x2 that of THP, a0 = −2.4697 cm3 mol−1, and a1 = 0.0608 cm3 mol−1. The density of propionic acid at this temperature is 0.971 74 g cm−3; that of THP is 0.863 98 g cm−3. (a) Derive an expression for the partial molar volume of each component at this temperature. (b) Compute the partial molar volume for each component in an equimolar mixture.