When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
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When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the...
A solution contains 10.35 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -3.26 ∘C. The mass percent composition of the compound is 60.98% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?
A solution contains 11.70 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -7.01 ∘C. The mass percent composition of the compound is 38.70% C, 9.74% H, and the rest is O. What is the molecular formula of the compound? Express your answer as a molecular formula So far I got CH3O as my empirical, but I can't seem to figure out how...
A solution containing 1.00 g of an unknown non-electrolyte liquid and 9.00 g water has a freezing point of -3.33 oC. The Kf = 1.86 oC/m for water. Calculate the molar mass of the unknown liquid, in g/mol.
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...
A student is determining the molar mass of an unknown compound based on the following data: mass compound: 4.80 g mass solvent (water): 0.022 kg new freezing point: -2.50 oC freezing point depression constant (Kf): 1.86 oC/molal (Freezing point of pure water = 0 oC) 0.0786 g/mol 162.33 g/mol 0.00616 g/mol 293.26 g/mol
0.2650 g of a compound of unknown molecular mass were dissolved in 18.00 mL of a non-ionizing solvent with specific gravity of 0.7480. The pure solvent was determined to have a freezing point of 6.80°C. The freezing point of the solution was determined graphically. Trial one yielded a freezing point of 5.31°C for the solution. Trial two indicated the freezing point to be 5.23°C. Kf (solvent) = 12.8 C°/m a. Calculate the molecular mass of the unknown. b. If 5.50...
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute? 1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the...
Determine the molar mass of an unknown non-electrolyte compound given the following data: 1.453 grams of the unknown compound is dissolved in 10.08 grams of water (Kf = 1.853 0C/m). The solution freezes at -1.47 0C. What is the molar mass of the unknown compound?
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
The freezing point of a solution that contains 1.00 g of an unknown compound, (A), dissolved in 10.0 g of benzene is found to be 2.17 oC. The freezing point of pure benzene is 5.48 oC. The molal freezing point depression constant of benzene is 5.12 oC/molal. What is the molecular weight of the unknown compound?