The normal freezing point of a certain liquid X is 4.60°C, but when 40.g of iron(III) nitrate (FeNO33) are dissolved in 350.g of X the solution freezes at 3.7°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Be sure your answer is rounded to the correct number of significiant digits.

[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit

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

How many grams of pentane, CH3(CH2)3CH3, must be mixed with 64.18 g of hexane, CH3(CH2)4CH3, at 25.00 °C to produce a solution with a vapor pressure above the solution of 273.5 torr? The vapor pressures of pure pentane and hexane at 25.00 °C are 511.0 torr and 150.0 torr, respectively. These compounds form nearly ideal solutions when mixed together.

A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant K=3.91 °C·kgmol . Calculate the freezing point of a solution made of 146.g of iron(III) chloride (FECI,) dissolved in 900. g of X. Round your answer to 3 significant digits.

A certain substance X has a normal freezing point of 4.7 °C and a molal freezing point depression constant K₁ = 3.86 °C · kg • mol by dissolving some urea ((NH,),CO) in 600. of X. This solution freezes at 1.3 °C. Calculate the mass of urea that was dissolved. Be sure your answer has the correct number of significant digits. g ☐ x10 X 1 . A solution is prepared 5

The normal boiling point of a certain liquid X is 140.50 °C, but when 32.3 g of alanine (C,H,NO,) are dissolved in 250. g of X the solution boils at 141.7 °C instead. Use this information to calculate the molal boiling point elevation constant K, of Х. Round your answer to 2 significant digits. olo °C·kg Ar K, = [] mol

When 2.01 g of a certain molecular compound X are dissolved in 50.0 g of benzene (CH), the freezing point of the solution is measured to be 4.9 °C. Calculate the molar mass of X. 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 1 significant digit. 0 ロ・ロ X x10

The molal boiling point elevation constant =Kb·0.53°C·kgmol−1 for a certain substance X. When 7.3g of urea NH22CO are dissolved in 200.g of X, the solution boils at 120.5°C. Calculate the boiling point of pure X. Round your answer to 4 significant digits.