Textbook Question
At 60 °C, compound X has a vapor pressure of 96 mm Hg, benzene 1C6H62 has a vapor pressure of 395 mm Hg, and a 50:50 mixture by mass of benzene and X has a vapor pres- sure of 299 mm Hg. What is the molar mass of X?
Ch.13 - Solutions & Their Properties
Chapter 13, Problem 144
Elemental analysis of b@carotene, a dietary source of vitamin A, shows that it contains 10.51% H and 89.49% C. Dissolving 0.0250 g of b@carotene in 1.50 g of camphor gives a freezing- point depression of 1.17 °C. What are the molecular weight and formula of b@carotene? [Kf for camphor is 37.7 1°C kg2>mol.]
Verified step by step guidance1
First, let's determine the empirical formula of b@carotene. The empirical formula is the simplest whole number ratio of atoms in a compound. Given the percentages of hydrogen (H) and carbon (C), we can assume a 100g sample. This means we have 10.51g of H and 89.49g of C. Convert these masses to moles by dividing by the atomic masses of H (1.01 g/mol) and C (12.01 g/mol).
Next, divide the number of moles of each element by the smallest number of moles calculated in the previous step. This will give you the ratio of atoms in the empirical formula.
Now, let's find the molecular weight of b@carotene. We can use the freezing point depression of the solution and the formula ΔTf = Kf * m, where ΔTf is the freezing point depression, Kf is the cryoscopic constant, and m is the molality of the solution. The molality can be calculated as moles of solute divided by kilograms of solvent.
Using the molality and the mass of b@carotene, we can calculate the moles of b@carotene. Then, divide the mass of b@carotene by the moles to get the molecular weight.
Finally, divide the molecular weight by the empirical formula weight (which can be calculated from the empirical formula obtained in step 2). If this number is close to a whole number, multiply the subscripts in the empirical formula by this number to get the molecular formula of b@carotene.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Freezing Point Depression
Freezing point depression is a colligative property that describes the lowering of a solvent's freezing point when a solute is added. The extent of this depression is directly proportional to the number of solute particles in the solution. The formula used to calculate freezing point depression is ΔTf = Kf * m, where ΔTf is the change in freezing point, Kf is the freezing point depression constant of the solvent, and m is the molality of the solution.
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Freezing Point Depression
Molecular Weight Calculation
Molecular weight, or molar mass, is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To determine the molecular weight of a compound, one must first find the number of moles of solute using the freezing point depression data and the known Kf value. Once the moles are calculated, the molecular weight can be found by dividing the mass of the solute by the number of moles.
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Empirical and Molecular Formulas
The empirical formula represents the simplest whole-number ratio of elements in a compound, while the molecular formula indicates the actual number of atoms of each element in a molecule. To derive the molecular formula from the empirical formula, one must determine the molar mass of the compound and compare it to the molar mass of the empirical formula. This comparison helps in identifying the factor by which the empirical formula must be multiplied to obtain the molecular formula.
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Textbook Question
Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dissolving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (b) What mass of MClx is formed? (a) How many moles of H2 gas are evolved?