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.
A solution containing 1.00 g of an unknown non-electrolyte liquid and 9.00 g water has a...
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.
A solution is prepared by dissolving 11.10 g of an unknown non-electrolyte solute in 78.64 g of cyclohexane. The freezing point of the solution is found to be 2.06 oC. What is the molar mass of the unknown solute in g/mol? Please report your answer with 3 significant figures. Answer g/mol
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...
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...
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)?
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?
An aqueous solution containing 15.0 g of an unknown molecular (nonelectrolyte) compound in 100.5 g of water has a freezing point of -1.9 ∘C. Calculate the molar mass of the unknown compound. I am stumped because I am not given 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 containing 0.16 g of an unknown electrolyte in 2.50 g of cyclohexane was found to freeze at 4.9 oC . What is the molar mass of the unknown substance?
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