The boiling point of diethyl ether, CH3CH₂OCH₂CH3, is 34.500 °C at 1 atmosphere. Kö(diethyl ether) 2.02 °C/m In a laboratory experiment, students synthesized a new compound and found that when 11.39 grams of the compound were dissolved in 297.6 grams of diethyl ether, the solution began to boil at 34.768 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? g/mol

The boiling point of diethyl ether, CH3CH₂OCH₂CH3, is 34.500 °C at 1 atmosphere. Kö(diethyl ether) 2.02 °C/m In a laboratory experiment, students synthesized a new compound and found that when 11.39 grams of the compound were dissolved in 297.6 grams of diethyl ether, the solution began to boil at 34.768 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound ? g/mol

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

A chemistry student weighs out 0.084 of an unknown solid compound X and adds it to 350. mL of distilled water at 23. C. After 10 minutes of stirring, only some of the X has dissolved. The student drains off the solution, then washes, dries and weighs the X that did not dissolve. It weighs 0.042 kg. Using only the information above, can you calculate the solubility of Xin water at 23.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. 0 yes no x10 ロ・ロ X 00
Complete combustion of 10.98 g of a compound of carbon, hydrogen, and oxygen yielded 16.10 g CO2 and 6.592 g H₂O. When 6.780 g of the compound was dissolved in 261 g of water, the freezing point of the solution was found to be -0.805 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
The solubility of PbCrO4 in water at 25 °C is measured to be 1.7 × 10° Round your answer to 2 significant digits. D ] x16 × -4 g L Use this information to calculate Ksp for PbCrO4.
A pharmacist mixes togehter 20 g of crystals of compound A and 10g of crystals of compound B. The mixture is then dissolved in 120mL of water to make cough syrup.
A chemistry student is given 5.00 L of a clear aqueous solution at 25.° C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 15.° C. At that point, the student sees that a precipitate has formed. He transfers the liquid to a clean new beaker and throws away the precipitate. The student then evaporates the water from the liquid in the new beaker under vacuum. It weighs 1.00 kg. Using only the information above, can you calculate the solubility of Xin water at 15.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. 0 yes no ☐ x10 X Olo S U 2
Complete combustion of 8.653 g of a compound of carbon, hydrogen, and oxygen yielded 21.83 g CO₂ and 3.831 g H₂O. When 18.00 g of the compound was dissolved in 288 g of water, the freezing point of the solution was found to be -0.952 °C. For water, Kfp = = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
The boiling point of water, H₂O is 100.00 °C at 1 atmosphere and its Kpp value is 0.512 °C/m. A nonvolatile, nonelectrolyte that dissolves in water is sucrose. How many grams of sucrose, C12H22O11 (342.3 g/mol), must be dissolved in 208.0 grams of water to raise the boiling point by 0.350 °C? g sucrose.
A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.
(Q65) Calculate the vapor pressure (in torr) at 30°C of a solution containing 155.1 grams of the nonelectrolyte glucose (C6H1206) dissolved in 821.4 grams of water. The vapor pressure of pure water at this temperature is 31.80 torr. (4 sf)
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 boiling point of benzene, C6H₁, is 80.100 °C at 1 atmosphere. K₁ (benzene) = 2.53 °C/m In a laboratory experiment, students synthesized a new compound and found that when 11.45 grams of the compound were dissolved in 248.8 grams of benzene, the solution began to boil at 80.428 °C. The compound was also found to be nonvolatile and a non- electrolyte. What is the molecular weight they determined for this compound? || g/mol
A certain liquid X has a normal boiling point of 105.30°C and a boiling point elevation constant =Kb1.13·°C·kgmol−1 . Calculate the boiling point of a solution made of 52. g of zinc chloride ( ZnCl2 ) dissolved in 450.g of X .