When 147. g of urea (CH4N₂O): are dissolved in 1350. g of a certain mystery liquid X, the freezing point of the solution is 4.40 °C less than the freezing point of pure X. Calculate the mass of sodium chloride that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i= 1.68 for sodium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. 0 010 ロ・ロ

Suppose that you add 21.1 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 °C/m. With the added solute, you find that there is a freezing point depression of 2.86 °C compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound?

When 2.85 g of a certain molecular compound X are dissolved in 85. g of dibenzyl ether ((CH₂CH₂)₂O), the freezing point of the solution is measured to be 2 -1.2 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. X x10 Ś

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?

The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?

A solution is made by dissolving 0.645 mol of nonelectrolyte solute in 761 g of benzene. Calculate the freezing point, Tf, and boiling point, Th, of the solution. Constants can be found in the table of colligative constants. Tf= Tb = °C °C

The normal boiling point of methanol is 64.7°C. A solution containing a nonvolatile solute dissolved in methanol has a vapor pressure of 670. torr at 64.7°C. What is the mole fraction of methanol in this solution? Mole fraction =

A solution is made by dissolving 0.563 mol of nonelectrolyte solute in 821 g of benzene. Calculate the freezing point, Tf, and boiling point, Tp, of the solution. Constants can be found in the table of colligative constants. T = 1.97896467722 °C 78.3650548112 °C Incorrect

Biphenyl, C1,H10, is a nonvolatile, nonionizing solute that soluble in benzene, C,H6. At 25 °C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 17.8 g of biphenyl in 30.3 g of benzene? Psolution Torr II

1. Suppose that you add 27.5 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 3.58 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound? 2. What is the freezing point (in degrees Celcius) of 3.70 kg of water if it contains 187.4 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. 3. What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -5.6 °C? The freezing point depression constant of water is 1.86 ºC/m.