A solution containing 0.20 g of an unknown non-electrolyte in
2.50 g of cyclohexane was found...
A solution containing 0.20 g of an unknown non-electrolyte in
2.50 g of cyclohexane was found to freeze at 4.5 oC . What is the
molar mass of the unknown substance?
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An aqueous solution containing 34.1 g of an unknown molecular
(non-electrolyte) compound in 159.9 g of water was found to have a
freezing point of -1.5 ∘ C Calculate the molar mass of the unknown
compound.
a solution is made by mixing 1.08 g of an unknown non-volatile
non-electrolyte with 10.0 g of benzene. The freezing point of pure
benzene is is 5.5 degrees Celsius. The molal freezing point
depression constant, Kf, for benzene is 5.12 degrees Celsius per
molale.
What is the value of the freezing point depression? What is the
molality of the solution? What is the molar mass of the
unknown?
A solution contains 12.00 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
-4.95 ∘C. The mass percent composition of the compound is 53.31% C,
11.19% H, and the rest is O. Part A What is the molecular formula
of the compound? Express your answer as a molecular formula.
When 1.31 g of an unknown non-electrolyte is dissolved in 50.0 g
of acetone, the freezing point decreased to -94.1 degrees C from
-93.4 degrees C. If the Kfp of the solvent is 2.4 K/m, calculate
the molar mass of the unknown solute
A solution containing 34.2 g of cane sugar (C12H22O11 ) in 500.0
g of an unknown solvent froze at –0.374°C.
Calculate the freezing point depression constant of the solvent.
Calculate the molar mass of cane sugar.
A solution containing .40249 g of CoCl2 *
xH2O ( a solid with an unknown number of waters of
hydration) was exhaustively electrolyzed to deposit .09937 g of
metallic cobalt on a platinum cathode by the reaction
Co2+ + 2e- ---> Co(s). Calculate the
number of moles of water per mole of cobalt in the reagent.
An aqueous solution containing 15.9 g of an unknown molecular
(nonelectrolyte) compound in 106.5 g of water was found to have a
freezing point of -2.0 ∘C.
Calculate the molar mass of the unknown compound.
The osmotic pressure of a solution containing 1.44 g of an
unknown compound dissolved in 175.0 mL of solution at 25 ∘C is 1.93
atm. The combustion of 32.88 g of the unknown compound produced
55.60 gCO2 and 22.76 gH2O. What is the molecular formula of the
compound (which contains only carbon, hydrogen, and oxygen)?
Express your answer as a chemical formula.
The osmotic pressure of a solution containing 1.02 g of an
unknown compound dissolved in 175.0 mL of solution at 25 ∘C is 1.93
atm. The combustion of 23.40 g of the unknown compound produced
41.70 gCO2 and 17.07 gH2O. What is the molecular formula of the
compound (which contains only carbon, hydrogen, and oxygen)?
The osmotic pressure of a solution containing 1.44 g of an
unknown compound dissolved in 175.0 mL of solution at 25 ∘C is 1.93
atm . The combustion of 32.88 g of the unknown compound produced
55.60 gCO2 and 22.76 gH2O . What is the molecular formula of the
compound (which contains only carbon, hydrogen, and oxygen)?