The elemental analysis of an organic solid extracted from gum arabic (a gummy substance used in adhesives, inks, and pharmaceuticals) showed that it contained 40.0 percent by mass C, 6.7 percent by mass H, and 53.3 percent by mass O. A solution of 0.637 g of the solid in 32.9 g of the solvent diphenyl °C gave a freezing-point depression of 1.29 °C. Calculate the molar mass and molecular formula of the solid. (K, for diphenyl is 8.00 .) m Part 1 of 2 Round your answer to 3 significant digits. molar mass: Part 2 of 2 g mol molecular formula: X X 3

The elemental analysis of an organic solid extracted from gum arabic (a gummy substance used in adhesives, inks, and pharmaceuticals) showed that it contained 40.0 percent by mass C, 6.7 percent by mass H, and 53.3 percent by mass O. A solution of 0.637 g of the solid in 32.9 g of the solvent diphenyl °C gave a freezing-point depression of 1.29 °C. Calculate the molar mass and molecular formula of the solid. (K, for diphenyl is 8.00 .) m Part 1 of 2 Round your answer to 3 significant digits. molar mass: Part 2 of 2 g mol molecular formula: X X 3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The elemental analysis of an organic solid extracted from gum arabic (a gummy substance used in adhesives, inks, and pharmaceuticals) showed that it contained 40.0 percent by mass C, 6.7 percent by mass H, and 53.3 percent by mass O. A solution of 0.705 g of the solid in 31.9 g of the solvent diphenyl °C gave a freezing-point depression of 1.47 °C. Calculate the molar mass and molecular formula of the solid. (K, for diphenyl is 8.00- .) m Part 1 of 2 Round your answer to 3 significant digits. molar mass: Part 2 of 2 mol molecular formula: 2 NO 0 x10 X
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 1.50g of camphor gives a freezing-point depression of 1,17 degrees celsius. What are the molecular mass and formula of b-carotene? (Kf for camphor is 37.7(degrees celsius x kg)/mol.)
Calculate the vapor pressure of a solution containing 26.8 g of glycerin (C3H8O3) in 114 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic), and use a density of 1.00 g/mL for water. Express the pressure in torr to three significant figures. ►View Available Hint(s) Psolution = Submit IVE ΑΣΦ ? torr
Suppose that you add 21.1 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 °C/m. With the added solute, you find that there is a freezing point depression of 2.86 °C compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound?
The vapor pressures of ethanol (C₂H5OH) and 1-propanol (C3H₂OH) at 35 °C are 100. mmHg and 37.6 mmHg, respectively. Assume ideal behavior and calculate the partial pressures of ethanol and 1-propanol at 35 °C over a solution of ethanol in 1-propanol, in which the mole fraction of ethanol is 0.345. Be sure each of your answer entries has the correct number of significant digits. Part 1 of 2 P ethanol Part 2 of 2 P₁- 1- propanol mmHg mmHg x x10 X S Ś
Benzyl acetate is one of the active components of oil of jasmine. If 0.125 g of the compound is added to 25.0 g of chloroform (CHCl3), the boiling point of the solution is 61.82 °C. What is the molar mass of benzyl acetate?
Glycerin 1C3H8O32 is a nonvolatile nonelectrolyte with a density of 1.26 g>mL at 25 °C. Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 23.8 torr (Appendix B), and its density is 1.00 g>mL.
When 1.35 g of an unknown non-electrolyte is dissolved in 50.0 g of benzene, the freezing point decreased by 0.43 degrees C. If the Kfp of the solvent is 5.12 K/m, calculate the molar mass of the unknown solute.
The freezing-point depression constant for mercuric chloride, HgCl2, is 34.3K/m. A 0.849g sample of mercurous chloride, HgCl (empirical formula) dissolved in 50.0g of HgCl2 causes a freezing-point depression of 1.24K. What is the molecular formula for mercurous chloride? [Note: Mercuric chloride, HgCl2, the solvent in this case, is a mercury(II) compound, while mercurous chloride, HgCl, the solute, is a mercury(I) compound.]
The elemental analysis of an organic solid extracted from gum arabic (a gummy substance used in adhesives, inks, and pharmaceuticals) showed that it contained 40.0 percent by mass C, 6.7 percent by mass H, and 53.3 percent by mass O. A solution of 0.665 g of the solid in 23.5 g of the solvent diphenyl gave a freezing-point depression of 1.89 °C. Calculate the molar mass and molecular formula of the solid. (K; °C for diphenyl is 8.00.) m Part 1 of 2 Round your answer to 3 significant digits. molar mass: Part 2 of 2 D₁ g mol molecular formula: Do X 0x10 X
When 20.0 grams of an unknown nonelectrolyte (i=1) compound are dissolved in 500.0 grams of benzene, the freezing point of the resulting solution is 3.77 °C. The freezing point of pure benzene is 5.444 °C and the Kf for benzene is 5.12 °C/m. What is the molar mass of the unknown compound?
For ideal salt solutions, the freezing point depression is expressed as ∆T = iK , where is the number ofions in the salt. For example, NaCl has i = 2. Calculate how much NaCl (in %w/w) is required to lower thefreezing point of water to −9.00 °C. (this is used in ice cream making)Kf = 1. 86 deg kg mol^−1 a. Calculate the molality needed for ∆T = 9. 00 °C.b. Convert this molality into %(w/w) using MMNaCl = 58. 44 g/mol