The boiling point of diethyl ether, CH3CH2OCH2CH3, is 34.500 °C at 1 atmosphere. Kb(diethyl ether) = 2.02 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 14.04 grams of the compound were dissolved in 299.9 grams of diethyl ether, the solution began to boil at 35.025 °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 benzene, C6H6 , is 80.100 °C at 1 atmosphere. Kb (benzene)= 2.53C/m. In a laboratory experiment, students synthesized a new compound and found that when 14.93 grams of the compound were dissolved in 252.2 grams of benzene, the solution began to boil at 80.619 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound?   The freezing point of ethanol, CH3CH2OH, is -117.300 °C at 1 atmosphere. Kf(ethanol) = 1.99 °C/m. In a laboratory experiment, students synthesized a new compound and found that when 12.91 grams of the compound were dissolved in 271.5 grams of ethanol, the solution began to freeze at -117.406 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound?

(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)

The freezing point of pure benzene (CoHo) is 5.49 °C. The freezing point of a solution made using toluene (C-Hs) in benzene is determined to be -13.0 °C. What is the molality of the toluene? (Kf benzene = 5.12 °C/m)

An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 °C. What is the average molar mass of starch? (Becausenot all starch molecules are identical, the result will be an average.)   What is the freezing point of the solution?   Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)

The freezing point of water, H2O, is 0.000 °C at 1 atmosphere. Kf(water) = 1.86 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 11.94 grams of the compound were dissolved in 217.1 grams of water, the solution began to freeze at -1.702 °C. The compound was also found to be nonvolatile and a non-electrolyte.What is the molecular weight they determined for this compound?

The boiling point of diethyl ether, CH3 CH₂ OCH2 CH3, is 34.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is chlorophyll. A student dissolves 11.24 grams of chlorophyll, C55 H72 MgN4O5 (893.5 g/mol), in 249.4 grams of diethyl ether. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂OH CHC13 C6H6 Diethyl ether CH3 CH₂ OCH₂ CH3 The molality of the solution is The boiling point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12

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 92.90°C and a boiling point elevation constant Kb=2.15·°C·kgmol−1. Calculate the boiling point of a solution made of 30.g of potassium bromide (KBr) dissolved in 800.g of X. Round your answer to 3 significant digits.

1 A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K = 5.78 °C·kg⋅mol A solution is prepared by dissolving some glycine (C₂HÃNO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂H²NO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. 1 g | x10 S