2. A solution of an unknown molecular substance is prepared by dissolving 0.50 g of the...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. b) The molality of the solution is 3.63. How many moles of the unknown compound were dissolved in the solution? C) what is the molar mass of the unknown compound?
Colligative properties, need to calculate the molar mass of the unknown substance: Can you please show the work for this problem? Thanks! 13 A solution was prepared by dissolving 59.82 g of an unknown (non-ionic) substance to 100.0 g of water. The boiling point of this solution was measured to be 101.7°C. unknown substance. Determine the molar mass of the 13 A solution was prepared by dissolving 59.82 g of an unknown (non-ionic) substance to 100.0 g of water. The...
1. A solution was prepared by dissolving 2.20g of urea (H2NCONH2) in 50.00g of water. If for H2O Tb = 100C, Tf = 0C, Kb = 0.52C / m and Kf = 1.86C / m, determine the freezing and boiling point of the solution. 2. A solution is prepared by dissolving 17.41g of a substance X in 600g of benzene and the resulting solution is frozen at 4.00C. If the freezing point of pure benzene is 5.55C and its Kf...
A solution is prepared by dissolving 3.04 g of an unknown nonelectrolyte in 16.00 g of cylcohexane (tf = 6.6 oC and kf = 20.0 oC/m). What is the molar mass of the unknown compound if the solution has a freezing point of -6.7 oC? Please see https://youtu.be/lwWZ5hdB61M for assistance. Mm = g/mol
A solution is prepared by dissolving 0.107 g of an unknown non-electrolyte in 88.1 g of camphor. The freezing point of the solution was measured to be 178.0�C. What is the molecular weight of the compound? (The freezing point of pure camphor is 179.5�C and kf= 40�C/m)?
The freezing point of a solution of 1.104 g of an unknown nonelectrolyte dissolved in 36.81 g of benzene is 1.08°C. Pure benzene freezes at 5.48°C and its Kf value is 5.12°C/m. What is the molecular weight of the compound?
8) Dissolving 7.75 g of a substance into 825 g of benzene at 298 K raises the boiling point by 0.575 K. Given that K, = 5.12 K kg mol-1 and K) = 2.53 K kg mol-1, calculate the freezing point depression, the molar mass of the solute, and the mole fraction of benzene in the solution.
Question #2 -/1 points How many grams of calcium nitrate need to be dissolved in 75 mL of water to form a solution that has a freezing point of -3.2 deg C? grams of calcium nitrate Evaluate Question #3 -/1 points What is the freezing point in °C) of a solution of 8.0 g of carbon tetrachloride, CCl4, in 80.0 g of benzene, C6H6. For benzene, Tp = 5.5°C and Kf = 5.12 deg kg mole?? Freezing point of solution...
. 0.275 L of solution is prepared by dissolving 2.50 g of an unknown molecular compound in enough water. The osmotic pressure of this solution is 1.98 atm at 27 °C. (R = 0.08206 L·atm/mol·K) a) Determine the molar mass of the molecular compound. (7 pts) b) If you need to prepare 0.275 L of AlCl3 solution with the same osmotic pressure of the above solution, what mass of AlCl3 (MW = 133.33 g/mol) would you need to weigh out?