(a) Eugenol is one of the compounds responsible for the flavor of cloves. A 111 mg sample of eugenol was dissolved in 1 g of chloroform (Kb =3.63°C/m), increasing the boiling point of the chloroform by 2.45°C. Calculate eugenol's molar mass. Eugenol is 73.17% C, 7.32% H, and 19.51% O by mass. What is the molecular formula of eugenol?

(a) Eugenol is one of the compounds responsible for the flavor of cloves. A 111 mg sample of eugenol was dissolved in 1 g of chloroform (Kb =3.63°C/m), increasing the boiling point of the chloroform by 2.45°C. Calculate eugenol's molar mass. Eugenol is 73.17% C, 7.32% H, and 19.51% O by mass. What is the molecular formula of eugenol?

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

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 40E: In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would...

See similar textbooks

Similar questions

H2. A solution contains 100.0 g water, 10.0 g NaCI, and 15.0 g methanol. What is the weight percentage of methanol in the solution? Please give typed answer
The normal freezing point of water, H2O is 0.00 °C and its Kfp value is 1.86°C/m.Assuming complete dissociation of the electrolyte, if 10.48 grams of potassium nitrate (KNO3, 101.1 g/mol) are dissolved in 271.7 grams of water what is the freezing point of the solution?Answer: ____ °C
a solution of 4.57 g carminin acid (H9C22H11O13 m.w. 492.4 g/mol, a coloring agent used in food, derived from the insect cochineal), and an electrolyte was dissolved in 6.47 g ethanol. What is the freezing point of the solution? (Correct ANS: -142.6, please show all work)
What is the freezing point (in degrees Celcius) of 3.97 kg of water if it contains 151.6 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. Type answer:
How do you solve? The freezing point depression constant for benzene is 5.06 °C/m and the freezing point of pure benzene is 5.51°C. If a solution containing 3.241 g of a solid dissolved into 50.0 g of benzene has a freezing point of 4.68°C, what is the molar mass of the solid? Make sure units are correct and sig figs.
c An aqueous KBr solution has a mole fraction, X, equal to 0.286. What is the molality of this solution? Express your answer to three significant figures. m = Answer m
The normal freezing point of water, H2O is 0.00 °C and its Kfp value is 1.86°C/m.Assuming complete dissociation of the electrolyte, if 11.48 grams of manganese(II) chloride (MnCl2, 125.8 g/mol) are dissolved in 231.4 grams of water what is the freezing point of the solution? Answer: _____ °C
The normal boiling point of water, H2O is 100.00 °C and its Kbp value is 0.512 °C/m. Assuming complete dissociation of the electrolyte, if 13.47 grams of cobalt(II) chloride (CoCl2, 129.8 g/mol) are dissolved in 150.7 grams of water, what is the boiling point of the solution? Answer: ____ °C
The normal freezing point of ethanol (CH3CH2OH) is -117.300 °C and its Kfp value is 1.99 °C/m. In a laboratory experiment, students synthesized a new compound and found that when 10.50 grams of the compound were dissolved in 281.0 grams of ethanol, the solution began to freeze at -117.558 °C. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molecular weight they determined for this compound? Answer: ______g/mol
The freezing point of pure water is 0.0°C. How many grams of ethylene glycol (C2H6O2) must be mixed in 100.0 g of water to lower the freezing point of the solution to -4.3°C? (___ANSWER___) g
What will be the new vapor pressure of the water in a 100 mL solution of 10 g of sugar (MW= 1342.3 g/mol) with a density of 1.04 g/ml? The Vapor pressure of water ins 23.8 mmHg at 25oC. answer in 2 decimal places no need to write the unit
Activity 1. Solve Me! Calculate the problems below. Write your solution and box your finalanswer. Follow the flow of solving like the examples given above. You may use the K b and K fof water in the examples. 1. Calculate the freezing and boiling points of a solution prepared by dissolving 15.5 gof Al (NO 3 ) 3 in 200.0 g of water. (Molar mass of Al (NO 3 ) 3 is 212.996 g/mol). 2. A solution is prepared by dissolving 120 grams of NaCl in 450 grams of water. Findthe freezing and boiling points of this solution. (Molar mass of NaCl is 58.44 g/mol) Activity 2. Know Me! Look for a book or search the web for additional information regardingthe colligative properties of solution. Refer to the guide questions below. 1. State the effect that dissolving a solute has on each of the following physicalproperties of a solvent.a. Boiling pointb. Freezing point