When 552. g of benzamide (C,H,NO) are dissolved in 1000. g of a certain mystery liquid X, the freezing point of the solution is 8.3 °C lower than the freezingpoint of pure X. On the other hand, when 552. g of ammonium chloride (NH4C1) are dissolved in the same mass of X, the freezing point of the solution is31.6 °C lower than the freezing point of pure X.Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.= 0x10

Answered: When 552. g of benzamide (C,H,NO) are…

Chemistry

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Chapter1: Chemical Foundations

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When 153. g of glycine (C,H,NO2) are dissolved in 1400. g of a certain mystery liquid X, the freezing point of the solution is 4.9 °C lower than the freezing point of pure X. On the other hand, when 153. g of iron(III) nitrate (Fe(NO,)) are dissolved in the same mass of X, the freezing point of the solution is 4.8 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i = |
7 8. When 70.2 g of glycine (C, H,NO,) are dissolved in 900. g of a certain mystery liquid X, the freezing point of the solution is 3.7 °C lower than the freezing point of pure X. On the other hand, when 70.2 g of ammonium chloride (NH, Cl) are dissolved in the same mass of X, the freezing point of the solution is 9.0 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i= 1 Submit Assignment Continue Accessibility O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center II Finder F11 F12 F9 F10
When 225. of urea (CH,N,0) are dissolved in 1200. g Oof a certain mystery g liquid x, the freezing point of the solution is 8.4 °c lower than the freezing point of pure x. On the other hand, when 225. g of sodium chloride are dissolved in the same mass of x, the freezing point of the solution is 14.5 °C lower than the freezing point of pure x. olo Ar Calculate the van't Hoff factor for sodium chloride in x. Be sure your answer has a unit symbol, if necessary, and is rounded to the correct number of significant digits. i = |
The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.Calculate the vapor pressure of the solution at 25 °C when 10.17 grams of aspirin, C9H8O4 (180.1 g/mol), are dissolved in 151.7 grams of diethyl ether.diethyl ether = CH3CH2OCH2CH3 = 74.12 g/mol.
The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide (BaOH2) are dissolved in 900.g of X the solution freezes at −1.6°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Round your answer to 2 significant digits.
When 224. mg of a certain molecular compound X are dissolved in 45.0 g of cyclohexane (C6H₁2), the freezing point of the solution is measured to be 6.5 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, 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.
When 4.18 g of a certain molecular compound X are dissolved in 45.0 g of benzene (C6H6), 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 the correct number of significant digits. □□ 品 5
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Ethylene glycol (EG), CH₂(OH)CH₂(OH), is a common automobile antifreeze. It is water soluble and fairly nonvolatile (b.p. 197 °C). Calculate the freezing point of a solution containing 651 g of this substance in 2505 g of water. Would you keep this substance in your car radiator during the summer? The molar mass of ethylene glycol is 62.01 g.
When 14.4 g14.4 g of an organic compound known to be 55.81% C55.81% C, 7.0% H7.0% H, and 37.17% O37.17% O by mass is dissolved in 825.8 g825.8 g of benzene, the freezing point is 4.80 ∘C4.80⁢ ∘C. The normal freezing point of benzene is 5.49 ∘C5.49⁢ ∘C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. ?fKf values for various solvents are given in the colligative constants table. molecular formula: CHO
A solution made by dissolving 150.0 g of an unknown compound in 425.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. What was the molality of the solution? How many moles of the unknown compound were dissolved in the solution? What is the molar mass of the unknown compound?
1 A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K = 5.78 °C·kg⋅mol A solution is prepared by dissolving some glycine (C₂HÃNO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂H²NO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. 1 g | x10 S

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