When 221. g of glycine (c,H,NO,) are dissolved in 1100. g of a certain mystery liquid x, the freezing point of the solution is 6.10 °C less than the freezing point of pure x. Calculate the mass of ammonium chloride (NH,CI) that must be dissolved in the same mass of x to produce the same depression in freezing point. The van't Hoff factor i=1.62 for ammonium chloride in x. Be sure your answer has a unit symbol, if necessary, and is rounded to the correct number of significant digits. 몸

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.300 mol of liquid dibromoethane (C2H4Br2, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, P° = 173 torr).

Calculate the vapor pressure of a solution containing 26.8 g of glycerin (C3H8O3) in 114 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic), and use a density of 1.00 g/mL for water. Express the pressure in torr to three significant figures. ►View Available Hint(s) Psolution = Submit IVE ΑΣΦ ? torr

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

A solution is made by dissolving 0.540 mol of nonelectrolyte solute in 757 g of benzene. Calculate the freezing point, Tf, and boiling point, Tú, of the solution. Constants can be found in the table of colligative constants. Tf = Tb = °C °C

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

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.400 mol of liquid dibromoethane (C2H4Br2, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, P° = 173 torr).

At 25°C, the vapor pressure of pure benzene, C6H6, is 96.0 torr. The vapor pressure of pure ethanol, CH;OH, is 44.0 torr at the same temperature. Assuming ideal behavior, calculate the vapor pressure at 25°C of a solution that contains an equal mass of each.

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

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.250 mol of liquid dibromoethane (C2H4Br2, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, P° = 173 torr).