35.9 g of an unknown molecular (nonelectrolyte) compound dissolved in 150.0 g of benzene was found to have a freezing point of –1.3 °C. What is the molar mass of the unknown compound? The freezing point depression constant of benzene is 5.12 °C/m and it's normal freezing point is 5.50°C.

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The molal freezing point depression constant =Kf·7.96°C·kgmol−1 for a certain substance X. When 5.40g of urea NH22CO are dissolved in 200.g of X, the solution freezes at −4.9°C. Calculate the freezing point of pure X. Round your answer to 2 significant digits.

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The freezing point of benzene is 5.5 °C. What is the molar mass of a nonionizing solute if 1.911 grams of the solute added to 22.76 g of benzene lowers the freezing point to 3.37. The Kf of benzene is 5.12 °C/m.

A solution is made by dissolving 0.900g of compound Y into 11.000g of cyclohexane. The solution freezes at 3.9 oC. What is the molar mass of compound Y in g/mol?   The Freezing Point of Cyclohexane is 6.6oC. and the freezing point depression constant is kf = 20.0 oC/m. (m=molality). Group of answer choices 0.091 g/mol 606.06 g/mol 303.03 g/mol 1212.12 g/mol

When 105.g of glycine C2H5NO2 are dissolved in 1200.g of a certain mystery liquid X, the freezing point of the solution is 4.6°C lower than the freezing point of pure X. On the other hand, when 105.g of iron(III) chloride are dissolved in the same mass of X, the freezing point of the solution is 7.5°C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.      i=

3) A student weighed 1.75 g of an unknown molecular compound and dissolved it in 15 ml of water. The freezing point of the solution was measured to be -3.5 °C. Calculate the molar mass of the compound. (KF1.86 °C/m for water).

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

(CH), the freezing point of the solution is measured to be 3.5 °C. Calculate If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits. 0 When 11.5 g of a certain molecular compound X are dissolved in 45. g of benzene the molar mass of X. ロ・ロ X 0x1.2