freezing point is found to be -64.221°C for solution consisting of 10.5 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?
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?
Calculate the Freezing point of a solution containing 0.6 kg of chloroform, CHCL3, and 42.0 g of eucalptol, C10H18O. the normal freezing point of cholorform is (-63.5 c ) and the Kf IS 4.68 c/m
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...
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 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)?
Kf for chloroform is 4.68 C/m: normal freezing point go chloroform is -63.5 C. Calculate the freezing point of a solution containing 750 g of chloroform CHCL3 and 85 g of a solute that has a molar mass of 154 g/mol..
A) The vapor pressure of an aqueous solution of potassium bromide at 31 °C is 0.04173 atm. The vapor pressure of pure water at the same temperature is 0.04434 atm. Estimate the freezing point of the solution. For water, Kfp = 1.86 °C/m. Answer:_____ °C B) Complete combustion of 3.769 g of a compound of carbon, hydrogen, and oxygen yielded 8.120 g CO2 and 3.325 g H2O. When 13.90 g of the compound was dissolved in 253 g of water,...
The qualitative analysis of an organic compound showed C, H, O in combustion analysis of 0.20 34 g of a compound gave 0.5 911 g of CO2 and 0.10 36 g of H2O. the molecular weight of the compound was determined by the freezing point pressure method and was found in 210 from the above experimental results. determine the molecular formula of the compound 2. A compound is shown by qualitative analysis to contain carbon nitrogen oxygen and hydrogen combustion...
can y’all help me please? The freezing point of water, H2O, is 0.000 °C at 1 atmosphere. K(water)--1.86 °C/m In a laboratory experiment, students synthesized a new compound and found that when 12.51 grams of the compound were dissolved in 213.6 grams of water, the solution began to freeze at -1.813 °C. The compound was also found to be nonvolatile and a non-electrolyte What is the molecular weight they deterfnined for this compound ? g/mol The boiling point of chloroform,...