When 45.1 g of benzamlde (C,H,NOare dissolved In 850. g of a certaln mystery liquld X, the freezing point of the solutlon Is 7.70 °C less than the freezingpolnt of pure X.that must be dissolved In the same mass of X to produce the same depression In freezing point. The van't3/3)Calculate the mass of Iron(III) nitrate (Fe(NO.Hoff factor i=3.48 for Iron(III) nitrate in X.doBe sure your answer has a unit symbol, if necessary, and Is rounded to the correct number of significant digits.x102021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy AccessibiCheckExplanationM 9hp火

When 45.1 g of benzamlde (C,H,NO) are dissolved In 850. g of a certaln mystery liquld X, the freezing polnt of the solution Is 7.70 °C less than the freezing polnt of pure X. Calculate the mass of Iron(III) nitrate (Fe(NO,) that must be dissolved In the same mass of X to produce the same depression In freezing polnt. The van't Hoff factor i =3.48 for Iron(III) nitrate In X. Be sure your answer has a unit symbol, If necessary, and Is rounded to the correct number of slignificant digits. olo

When 45.1 g of benzamlde (C,H,NO) are dissolved In 850. g of a certaln mystery liquld X, the freezing polnt of the solution Is 7.70 °C less than the freezing polnt of pure X. Calculate the mass of Iron(III) nitrate (Fe(NO,) that must be dissolved In the same mass of X to produce the same depression In freezing polnt. The van't Hoff factor i =3.48 for Iron(III) nitrate In X. Be sure your answer has a unit symbol, If necessary, and Is rounded to the correct number of slignificant digits. olo

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

Calculate the mass of compound (molar mass = 256 g mol-1) to be dissolved in 75 g of benzene to lower its freezing point by 0.48 K (Kf = 5.12 K kg mol-1).
A solution consisting of 0.240 mol of methylbenzene, C6H5CH3, in 252 g of nitrobenzene, C6H5NO2, freezes at –0.7°C. Pure nitrobenzene freezes at 6.0°C. What is the freezing-point depression constant of nitrobenzene?
3. The vapor pressure over a solution of urea (CH4N₂O) is 291.2 mm Hg (PA). The vapor pressure of pure water at the same temperature is 355.1 mm Hg (PºA). Calculate the mole fraction of urea in the solution. [See above for MM(urea)]
The vapor pressure of benzene (C6H6) and toluene (C7H8) at 25 degrees Celcius are 95.1 and 28.4 mm Hg, respectively. A solution is prepared with a mole fraction of toluene of 0.550. What is the total vapor pressure above the solution?
When 142. g of alanine (C3H,NO2) are dissolved in 1500. g of a certain mystery liquid X, the freezing point of the solution is 7.30 °C less than the freezing point of pure X. Calculate the mass of iron(III) nitrate (Fe(NO3),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i=3.80 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. olo
I don’t know how to do this question
Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 ∘C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 11.4 g of biphenyl in 33.4 g of benzene?
A solution that contains 3.00 g of urea [CO(NH2)2] dissolved in 78.1 g of benzene (C6H6) has a freezing point of 2.37 C. The normal freezing point of benzene is 5.51 C. What is the freezing point depression constant for this solvent?
The vapor pressures of pure carbon disulfide and carbon tetrachloride are 360 and 99.8 Torr, respectively, at 296 K. What is the vapor pressure of a solution containing 63.5 g of each compound?
When 205. g of benzamide (C,H,NO) are dissolved in 550. g of a certain mystery liquid X, the freezing point of the solution is 2.50 °C less than the freezing point of pure X Calculate the mass of iron(111) nitrate (Fe(NO₂),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i-3.44 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. 10 of 0 0.0 cla 0.2 A
A solution prepared from 96 g of non-volatile non dissociating solute in 5.25 mole of toluene has a vapor pressure of 0.161 atm at 600C. What is the molecular weight of the solute? The vapor pressure of pure toluene at 600C is 0.184 atm.
Do not give handwriting solution.